Answer:
The change in cell potential under non-standard conditions can be predicted using the Nernst equation. The Nernst equation relates the measured cell potential to the reaction quotient and allows the accurate determination of equilibrium constants (including solubility constants).
In this case, the concentrations of Al³+ and Ni²+ are not standard. According to the Nernst equation, an increase in the concentration of the oxidizing agent ion in the cathodic side of the system (reduction reaction) should result in an increase in cell potential. Conversely, an increase in the concentration of the reducing agent in the anodic side of the system (oxidation reaction) should result in a decrease in cell potential.
Explanation:
The Nernst equation enables the determination of cell potential under non-standard conditions. It relates the measured cell potential to the reaction quotient and allows the accurate determination of equilibrium constants (including solubility constants).
The Nernst equation is given by:
Ecell = E°cell - (RT/nF)lnQ
where Ecell is the cell potential under non-standard conditions, E°cell is the standard cell potential, R is the universal gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred in the balanced equation for the cell reaction, F is Faraday’s constant, and Q is the reaction quotient.
At room temperature (25°C or 298K), this equation can be simplified to:
Ecell = E°cell - (0.0592/n)logQ
where logQ is the base-10 logarithm of the reaction quotient.
To calculate the change in cell potential using this equation, you need to know the standard cell potential (E°cell), the number of moles of electrons transferred in the balanced equation for the cell reaction (n), and the reaction quotient (Q) under non-standard conditions.
In a certain experiment, 0.969 mol sampe of Cu is allowed to react with 246mL of 6.60M HNO3 according to the following reaction:
Cu(s) + HNO3(aq) -> Cu(NO3)2(aq) + H2O + NO(g)
a) What is the limiting reactant?
b) How many grams of H2O is formed?
C) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
The moles of Nitric Acid present (1.6244 mol) is more than twice the moles of Cu (0.969 mol). Therefore, Copper is the limiting reactant. Therefore, 17.45 g of water is formed. Since we can't have negative moles.
How is the limiting reactant determined?The number of moles of each reactant can be calculated by dividing the volume of each solution by its molarity. You can identify which reactant is the limiting one in the balanced chemical equation by dividing the number of moles of each reactant by its stoichiometric coefficient.
a) Calculating the moles of copper and nitric oxide and comparing their stoichiometric ratios will help us identify the limiting reactant.
From the given information, the moles of Cu is 0.969 mol.
The moles of Nitric Acid can be calculated using the formula:
moles of Nitric Acid = (molarity) x (volume in liters)
moles of Nitric Acid = (6.60 mol/L) x (246/1000 L)
moles of Nitric Acid = 1.6244 mol
The balanced equation shows that 1 mol of Cu reacts with 2 mol of Nitric Acid.
The moles of Nitric Acid present (1.6244 mol) is more than twice the moles of Copper (0.969 mol). Therefore, Copper is the limiting reactant.
b)We can see from the balanced equation that 1 mol of Copper reacts to create 1 mol of water. As a result, the amount of Water generated will be 0.969 mol, which is identical to the amount of Copper that was reacted.
mass of water = moles of water x molar mass of water, where the molar mass of water is 18.015 g/mol.
mass of water = 0.969 mol x 18.015 g/mol
mass of water = 17.45 g (rounded to two decimal places)
Therefore, 17.45 g of water is formed.
c) Copper is the limiting reactant, hence no Nitric Acid will be completely oxidised. We must first figure out how many moles of Nitric Acid are needed to react with all of the Copper in order to compute how much extra Nitric Acid is still there.
From the balanced equation, we know that 1 mol of Cu reacts with 2 mol of Nitric Acid. Therefore, the moles of Nitric Acid required to react with 0.969 mol of Copper will be:
moles of Nitric Acid = 2 x 0.969 mol
moles of Nitric Acid = 1.938 mol
The initial moles of Nitric Acid present is 1.6244 mol. Therefore, the moles of excess Nitric Acid remaining after the reaction is:
moles of excess Nitric Acid = initial moles of Nitric Acid - moles of Nitric Acid required
moles of excess Nitric Acid = 1.6244 mol - 1.938 mol
moles of excess Nitric Acid = -0.3136 mol
Since we can't have negative moles, we know that all of the Nitric Acidwill be consumed, and there is no excess Nitric Acid remaining.
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Baliz reply asap, help indeed needed lol
In the SI system of units [International System of Units], the mole is one of seven base units. It is frequently used in chemical calculations. However, a mole of something is just a particular quantity of it. It is not a unit of measure in the way that meters, seconds, and kilograms are. Calculations performed with the number of moles of a substance could also be performed with the number of particles of a substance. Based on this information, do you think that the mole should be considered a base unit in the SI system? Explain why or why not.
Based on the information given, the mole should be considered a base unit in the SI system because it serves as a universally accepted measure of the amount or quantity of substances.
The mole is an amount unit similar to familiar units like pair, dozen, gross, etc. It provides a specific measure of the number of atoms or molecules in a bulk sample of matter.
A mole is defined as the amount of substance containing the same number of atoms, molecules, ions, etc. as the number of atoms in a sample of pure 12C weighing exactly 12 g.
SI units refer to units of measurement that are universally accepted for measuring the properties of quantities of objects.
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Calculate the heat change in joules for melting 12.0 g
of ice at 0 ∘C
The heat change required to melt 12.0 g of ice at 0°C is 4,002.6 joules.
To calculate the heat change in joules for melting 12.0 g of ice at 0°C, we need to use the specific heat of fusion of ice and the heat equation. The specific heat of the fusion of ice is 333.55 J/g.
The heat equation is:
Q = m × ΔH
where Q is the heat change, m is the mass of the substance, and ΔH is the specific heat of fusion.
Therefore, the heat change required to melt 12.0 g of ice at 0°C can be calculated as follows:
Q = 12.0 g × 333.55 J/g
Q = 4,002.6 J
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How many liter of CO2 gas at STP will contain 2136 molecules?
Answer: 2136 molecules of CO2 at STP will occupy a volume of 8.91 × 10^-24 L
Explanation:
STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 L of volume. Also, 1 mole of any gas contains 6.022 × 10^23 molecules.
1 mole of CO2 contains = 6.022 × 10^23 molecules
Therefore, 2136 molecules of CO2 will be present in a volume of:
= (1 mole CO2 / 6.022 × 10^23 molecules CO2) × (22.4 L / 1 mole CO2) × (2136 molecules CO2 / 1)
= 8.91 × 10^-24 L
A 49.0 g sample of water at 100. °C is poured into a 55.0 g sample of water at 25 °C. What will be the final temperature of the water? The specific heat of water is 4.184 J/g °C.
Final temperature =
How to balance this by oxidation state change method? . KMnO4 + KCl + H2SO4 --> K2SO4 + MnSO4+Cl2
To balance the given chemical equation using the oxidation state change method, we need to follow these steps:Step 1: Write the unbalanced equationKMnO4 + KCl + H2SO4 → K2SO4 + MnSO4 + Cl2
Step 2: Identify the elements that undergo oxidation and reductionIn this equation, the oxidation state of Mn changes from +7 to +2, which means it undergoes reduction, while the oxidation state of Cl changes from -1 to 0, which means it undergoes oxidation.
Step 3: Write the half-reactionsReduction half-reaction: MnO4^- → Mn^2+Oxidation half-reaction: Cl^- → Cl2Step 4: Balance the atoms and charges in each half-reactionReduction half-reaction: 8H+ + MnO4^- → Mn^2+ + 4H2OOxidation half-reaction: 2Cl^- → Cl2 + 2e^-Step 5: Balance the electrons in each half-reactionReduction half-reaction: 5e^- + 8H+ + MnO4^- → Mn^2+ + 4H2OOxidation half-reaction: 2Cl^- → Cl2 + 2e^-Step 6: Multiply each half-reaction by a factor to equalize the number of electrons transferredReduction half-reaction: 10e^- + 16H+ + 2MnO4^- → 2Mn^2+ + 8H2OOxidation half-reaction: 14Cl^- → 7Cl2 + 14e^-Step 7: Add the balanced half-reactions together10e^- + 16H+ + 2MnO4^- + 14Cl^- → 2Mn^2+ + 8H2O + 7Cl2Step 8: Cancel out the common terms on both sides of the equation2KMnO4 + 16KCl + 8H2SO4 → 2K2SO4 + 2MnSO4 + 7Cl2 + 8H2OTherefore, the balanced equation using the oxidation state change method is:2KMnO4 + 16KCl + 8H2SO4 → 2K2SO4 + 2MnSO4 + 7Cl2 + 8H2O.
Come up with at least two "crazy ideas" to explain the shape of the graph for difluoroethane.
Difluoroethane (DFE) is a cheap, commonly obtainable volatile chemical that is safe for recreational inhalation.
Thus, It can be found in everyday household items including propellants, refrigerants, and compressed air dusters. When breathed, DFE is a central nervous system (CNS) depressant that causes a momentary feeling of euphoria.
Toxic effects are linked to prolonged or excessive usage, and rapid termination might cause withdrawal.3–5 We describe a DFE misuse case that was accompanied by skeletal fluorosis and withdrawal psychosis.
Difluoroethane is a colourless, odourless gas that is transported under its vapour pressure as a liquefied gas. Ingestion of the liquid can result in frostbite.
Thus, Difluoroethane (DFE) is a cheap, commonly obtainable volatile chemical that is safe for recreational inhalation.
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At stp 22gm of CO2 gas occupies volume of
Explanation:
Use the Ideal Gas Law :
PV = n RT
STP = standard temp and pressure = 273.15 K and 1 atm
n = number of moles
CO2, (using table of elements) ,
has mole weight of 12.011 +2*15.999=~ 44 gm/mole
20 gm / 44gm/mole = .455 mole of CO2
R = gas constant = .082057 L atm /(K mole)
Plug in the numbers and solve for 'V'
(1 atm ) V = .455 * .082057 * 273.15
V = 10.2 liters
Here is another way:
....knowing that a mole of gas occupies 22.4 L /mole at STP
22.4 L / mole * .455 mole = ~10.2 liters
Among the elements of the main group, the first ionization energy increases
from left to right across a period.
from right to left across a period.
when the atomic radius increases.
down a group.
The first ionisation energy increases over time from left to right among the major group of elements. answer is option (a).
What is Ioniztion?When an element loses its valence electron, its oxidation number increases (a process known as oxidation), and this energy loss is known as ionisation (Ei).
Earth alkaline metals, which are located immediately next to alkaline metals, have higher ionisation energies than alkaline metals because they have two valence electrons, while alkaline metals, which are located far left in the main group, have the lowest ionisation energies and are easiest to remove.
Because they contain a large number of valence electrons, nonmetals are far to the right in the main group and have the highest ionisation energy.
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The complete question is,
Among the elements of the main group, the first ionization energy increases
a. from left to right across a period.
b. from right to left across a period.
c. when the atomic radius increases.
d. down a group.
Among the elements of the main group, the first ionization energy increases
from left to right across a period.
from right to left across a period.
when the atomic radius increases.
down a group.
The first ionisation energy increases over time from left to right among the major group of elements. answer is option (a).
What is Ioniztion?When an element loses its valence electron, its oxidation number increases (a process known as oxidation), and this energy loss is known as ionisation (Ei).
Earth alkaline metals, which are located immediately next to alkaline metals, have higher ionisation energies than alkaline metals because they have two valence electrons, while alkaline metals, which are located far left in the main group, have the lowest ionisation energies and are easiest to remove.
Because they contain a large number of valence electrons, nonmetals are far to the right in the main group and have the highest ionisation energy.
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The complete question is,
Among the elements of the main group, the first ionization energy increases
a. from left to right across a period.
b. from right to left across a period.
c. when the atomic radius increases.
d. down a group.
The specific heat capacity of benzene (C6H6) is 1.74 J/g*K. How much energy as heat is required to raise the temperature of 50.00 mL of benzene from 25.52 C to 28.75 C. Density of benzene is 0.876 g/cm3.
The amount of heat required is 246.165 Joules.
We can use the following method to figure out how much energy it will take to raise the temperature of benzene:
Q = mcΔT
Where Q = the amount of energy needed (in Joules).
m = the number of grams of benzene.
c = the amount of heat that benzene can hold (in J/g*K).
T = temperature change (in Kelvin)
But since the volume of benzene is given to us, we need to find the mass of Benzene by:
Density = mass/volume
mass = density x volume
mass = 0.876 g/cm3 x 50.00 mL = 43.8 g
Change in temperature = 28.75 - 25.52 = 3.23 K
Now, we can use the given numbers to fill in the formula for Q:
Q = mcΔT
Q = 43.8 g x 1.74 J/g*K x 3.23 K
Q = 246.165 J
So, it takes 238.92 Joules of heat energy to raise the temperature of 50 mL of benzene from 25.52°C to 28.75°C.
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Answer:
[tex]\Large \boxed{\boxed{\textsf{heat required = 246.2 J (4 s.f)}}}[/tex]
Explanation:
The heat energy required to raise the temperature of the reaction, i.e, the amount of heat energy released in the reaction (noting the rise in temperature, this is an exothermic reaction), can be calculated with the following calorimetry equation:
[tex]\Large \boxed{\textsf{$q=mc\Delta T$}} \sf \,, where:\\ \\\bullet q = quantity\,of\,heat\,released\,(measured\,in\,joules)\\ \bullet m = solvent\,of\,mass\,(measured\,in\,g\,or\,kg)\\\bullet c = specific\,heat\,capacity\,of\,solution\\\bullet \Delta T = change\,in\,temperature\,of\,solution[/tex]
To solve this, we know that:
[tex]\textsf{$\bullet$ m = 43.8 g (1 mL = 1 cm$^3$, using density = g/cm$^3$)}\\\textsf{$\bullet$ c = 1.74 J/g/K}\\\textsf{$\bullet \Delta T$ = 3.23 ($\Delta T$ is the same whether Kelvin or Celsius is used)}[/tex]
Inputting these values into the formula:
[tex]\large \textsf{$q = (43.8)(1.74)(3.23)$}\\ \\\large \textsf{$\therefore q=246.2$ J}\\ \\ \\\Large \boxed{\boxed{\textsf{$\therefore$ heat required = 246.2 J (4 s.f)}}}[/tex]
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1, The activation energy of the reaction is 71 KJ/Mol how many time is greater the rate constant for the reaction at temperature of 170°c and 150°c.
Answer:
cual es el propósito de este experimento
What is the rate of reaction (M/s) for the following process if the rate of change for NOBr was measured as -0.5 M/s.
2NOBr(g) ↔ 2NO(g) + Br2(g)
The rate of the reaction for the following process if the rate of change for NOBr was measured as -0.5 M/s. is 0.25 M/s.
The rate of a reaction is typically expressed as the rate of change of the concentration of a reactant or product over time. For the given reaction:
[tex]2NOBr(g)[/tex] ↔[tex]2NO(g)[/tex] [tex]+[/tex] [tex]Br_{2}[/tex](g)
The rate of the reaction can be expressed as:
[tex]rate = -1/2 * d[NOBr]/dt[/tex]
where [tex]d[NOBr]/dt[/tex] is the change in the concentration of NOBr over time, and the negative sign indicates that the concentration of NOBr is decreasing over time.
If the rate of change for NOBr was measured as -0.5 M/s, we can substitute this value into the above equation to find the rate of the reaction:
rate = -1/2 * (-0.5 M/s)
= 0.25 M/s
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What does it mean that water can ionize? Explain what this means if you could shrink down and see the true composition of water.
When water ionizes, it means that some of the water molecules break apart into ions, which are electrically charged particles. If you could shrink down and see the true composition of water at the molecular level, means water molecules are in a constant state of motion and interaction with each other.
Water (H₂O) is a polar molecule, meaning it has a partial positive charge on one end (hydrogen) and a partial negative charge on the other end (oxygen). This polarity allows water molecules to interact with each other through hydrogen bonding, which gives water its unique properties, such as high boiling and melting points, high heat capacity, and strong surface tension.
When water ionizes, it means that some of the water molecules break apart into ions, which are electrically charged particles. In the case of water, it can ionize into hydrogen ions (H⁺) and hydroxide ions (OH⁻);
H₂O → H⁺ + OH⁻
This ionization occurs when water molecules dissociate or separate into these charged particles due to the transfer of a proton (H⁺) between water molecules.
If you could shrink down and see the true composition of water at the molecular level, you would observe that water molecules are in a constant state of motion and interaction with each other. Some water molecules would be dissociating into hydrogen ions (H⁺) and hydroxide ions (OH⁻), while others would be recombining to form water molecules again.
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2Co + O2 = 2CO2
In this reaction 10.8 mole of carbon dioxide was produced .calculate the number of moles of carbon monoxide used in this reaction to produce such number of moles of carbon dioxide
Sonce the stoichiometric coefficients for both carbon dioxide and carbon monoxide are the same, the moles of CO2 formed and the moles of CO used are the same, therefore if 10,8 mole of carbon dioxide are being produced, then you would need 10,8 moles of carbon monozide
certain experiment, 0.969 mol sample of Cu is allowed to react with 246 mL of 6.60 M HNO3 according to the following action: મા
Cu(s) + HNO3(aq) → Cu(NO3)2(aq) + H2O(l) + NO(g)
Istan
a) What is the limiting reactant?
b) How many grams of H2O is formed?
c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
Copper is the limiting reactant, with n(Copper) = 0.969 mol being less than n(Nitric acid). It produces 17.44 grammes of water. As the outcome is negative, there is no excess Nitric acid. The reaction uses up all of the Nitric acid.
How are charges balanced in a redox reaction?The method described in the following steps can balance a redox equation: (1) Split the equation into two equal halves. (2) Make each half-mass reaction's and charge equal. (3) Ensure that the quantity of electrons going to each half-reaction is the same. The half-reactions should be combined.
n(Nitric acid) = (246 mL) x (6.60 mol/L) = 1.6236 mol
Since n(Copper) = 0.969 mol is less than n(Nitric acid), Copper is the limiting reactant.
m(Water) = n(Water) x M(Water) = 0.969 mol x 18.015 g/mol = 17.44 g
Therefore, 17.44 grams of Water is formed.
n(Nitric acid) needed = n(Copper) x 2 = 1.938 mol
The excess amount of Nitric acid is:
n(Nitric acid) excess = n(Nitric acid) initial - n(Nitric acid) needed
= 1.6236 mol - 1.938 mol
= -0.3144 mol
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41.6 g Al(NO3)3m Are added to a flask, how many liters of water should be added to create a 0.450 M solution?
To calculate the volume of water needed to create a 0.450 M solution of Al(NO3)3, we need to use the formula:
Molarity = moles of solute / volume of solution in liters
First, we need to determine the number of moles of Al(NO3)3 we have:
moles of Al(NO3)3 = mass / molar mass
molar mass of Al(NO3)3 = 1 x atomic mass of Al + 3 x atomic mass of N + 9 x atomic mass of O = 1 x 26.98 + 3 x 14.01 + 9 x 16.00 = 212.99 g/mol
moles of Al(NO3)3 = 41.6 g / 212.99 g/mol = 0.195 mol
Next, we can rearrange the formula above to solve for the volume of solution:
volume of solution = moles of solute / molarity
volume of solution = 0.195 mol / 0.450 M = 0.433 L
Therefore, we need to add 0.433 L (or 433 mL) of water to 41.6 g of Al(NO3)3 to create a 0.450 M solution.
Convert atm to Pa, using the numbers below
1.30 atmospheres is equivalent to 131723 pascal.
How to calculate atm to pascal?Atmospheres is a unit of measurement for pressure equal to 101325 Pa with symbol: atm.
Pascals, on the other hand, is the International System of Units (SI unit), the derived unit of pressure and stress, which is equivalent to one newton per square metre.
1 atmosphere = 101325 pascals
Therefore, 1.30 atm is equivalent to 1.3 × 101325 = 131723 Pa.
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1. What will be the final concentration of the solution indicated that will result from the
following dilutions?
a. 14.0 ml of a 4.2 M Na2CO3 solution is diluted to 86.0 ml.
Taking into account the definition of dilution, the final concentration of the solution is 0.68 M.
Definition of dilutionDilution is the process of reducing the concentration of solute in solution, which is accomplished by simply adding more solvent to the solution.
In a dilution the amount of solute does not change, but as more solvent is added, the concentration of the solute decreases, and the volume of the solution increases.
A dilution is mathematically expressed as:
Ci×Vi = Cf×Vf
where
Ci: initial concentrationVi: initial volumeCf: final concentrationVf: final volumeFinal concentrationIn this case, you know:
Ci: 4.2 MVi: 14 mLCf: ?Vf: 86 mLReplacing in the definition of dilution:
4.2 M× 14 mL= Cf× 86 mL
Solving:
(4.2 M× 14 mL)÷ 86 mL= Cf
0.68 M= Cf
In summary, the final concentration is 0.68 M.
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1. You have a calorimeter set up with 40 mL (40 g) of water. You perform chemical reaction and notice the temperature change of the water is 15°C. What is the energy change of the chemical reaction? (cwater= 4.18 J/g*°C)
2. You have set up a calorimeter using 50 mL (50 g) of water. When performing a chemical reaction with the calorimeter, you notice the temperature of the water changes from 25.0°C to 50.0°C. What is the energy released by the chemical reaction? (cwater=4.18 J/g*°C)
Heat capacity of a substance or system is defined as the amount of heat required to raise its temperature through 1°C. It is denoted by C. Heat capacity is an extensive property. Here the energy change is 2508 J.
The specific heat capacity of a substance is defined as the amount of heat required to raise the temperature of 1 gram of the substance through 1°C.
The heat required to raise the temperature of a sample of mass 'm' and specific heat capacity 'c' is:
q = mc ΔT
q = 40 × 4.18 × 15 = 2508 J
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metallic magnesium can be made by the electrolysis of molten MgCl2. how many minutes are needed to plate out 25g Mg from molten MgCl2 using 3.5 A of current?
Answer:
56,522 seconds = 942 minutes
Explanation:
n(Mg) = m/M(Mg) = 25 g / 24.31 g/mol = 1.03 mol of Mg
Q = n × 2 F = 1.03 mol × 2 × 96,485 C/mol = 197,820 C
t = Q / I = 197,820 C / 3.5 A = 56,522 s
When all the soil pores are essentially water-filled, flow is termed _______________ .
Unsaturated
Saturated
Gravitional
Rapid
If 0.250 mole of neon gas has a volume of 1520 mL at a pressure of 325 mmHg, what will be its
temperature in kelvins and in degrees Celsius? Show the rearranged ideal gas law solving for T. Cancel
units in work.
Answer:
Explanation:
We can use the ideal gas law to solve for the temperature of the neon gas:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, let's convert the volume from milliliters to liters:
V = 1520 mL = 1.52 L
Next, let's rearrange the ideal gas law to solve for T:
T = PV/nR
Now we can plug in the values and solve:
T = (325 mmHg)(1 atm/760 mmHg)(1.52 L)/(0.250 mol)(0.0821 L·atm/(mol·K))
T = 89.6 K
To convert to degrees Celsius, we subtract 273.15:
T = 89.6 K - 273.15 = -183.6 °C
Therefore, the temperature of the neon gas is 89.6 K or -183.6 °C.
CAN SOMEONE HELP WITH THIS QUESTION?
If the weight of Magnesium Metal is 0.6 g
1- FIND MOLES OF magnesium METAL
2- FIND CHANGE IN T CALORIMETER
3- Find q calorimeter
4- Find q reaction
5- Find the change in heat reaction per mole of Mg consumed
1- FIND MOLES OF magnesium METAL
Moles of Magnesium Metal = 0.6 g/24.31 g/mol = 0.0246 mol
What is Magnesium?Magnesium is a silvery-white alkaline earth metal that is a very abundant element in the Earth's crust. It is the eighth most abundant element in the universe.
2- FIND CHANGE IN T CALORIMETER
The change in temperature of the calorimeter is not given, so it cannot be calculated.
3- Find q calorimeter
The heat absorbed or released by the calorimeter is qcalorimeter = mCΔT, where m is the mass of the calorimeter, C is the specific heat capacity of the calorimeter, and ΔT is the change in temperature of the calorimeter. Since the mass and change in temperature of the calorimeter are not given, qcalorimeter cannot be calculated.
4- Find q reaction
The heat absorbed or released by the reaction is qreaction = nCΔT, where n is the number of moles of the reactant, C is the specific heat capacity of the reaction, and ΔT is the change in temperature of the reaction. Since the number of moles of the reactant and change in temperature of the reaction are not given, qreaction cannot be calculated.
5- Find the change in heat reaction per mole of Mg consumed
The change in heat per mole of Mg consumed is qMg = qreaction/n, where qreaction is the heat absorbed or released by the reaction and n is the number of moles of Mg. Since qreaction and n are not given, qMg cannot be calculated.
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Red light has a __________ wavelength than violet light
Red light has a longer wavelength than violet light. Wavelength is the distance between two consecutive peaks or troughs of a wave, and it determines the color of light. The range of visible light wavelengths is between approximately 400 nanometers (nm) for violet light to 700 nm for red light. So, red light has a longer wavelength and lower frequency than violet light.
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A 2135 ml sample of N₂ has a pressure of 95.4KPa at 135°C. What is the volume of the sample if temperature is
increased to 223°C and the pressure is kept constant?
B. 2595 ml
A. 913 ml
C. .3484 ml
D. 900 ml
Answer:
The correct answer is C: 3484 ml
what is chemical equitation
Answer:
A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and formulae, wherein the reactant entities are given on the left-hand side and the product entities on the right-hand side.
Explanation:
Good luck!
Answer:
A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and chemical formulas.
What is in a chemical equation?
A chemical equation (see an example below) consists of a list of reactants (the starting substances) on the left-hand side, an arrow symbol, and a list of products (substances formed in the chemical reaction) on the right-hand side.
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Fill the blanks
According to the Arrhenius definition, acids produce ---------------- ions when dissolved in water, and bases produce -------------------- ions when dissolved in water.
A) Protons, ammonium
b) Hydroxide, hydronium
C) ammonium, hydronium
d) hydronium, hydroxide
The Correct answer is D
Hydronium
hydroxide
ACTIVITY: SOLUTION CONCENTRATION VS. CONDUCTIVITY
Here is your goal for this lesson:
Graph experimental data and interpret results for peer review
A chemistry student carried out an experiment with a conducting apparatus (ammeter) similar to the one below. This ammeter measures in milliamperes (mA). The following data was taken.
Solution Reading
0.1 M H2SO4 150 mA
0.1 M Ba(OH)2 150 mA
To 30 mL of the Ba(OH)2 solution, 10 mL portions of H2SO4 were added until a total of
50 mL of H2SO4 were used. The following results were recorded.
DATA TABLE
Total H2SO4 Added Meter Reading Observations
0 mL 150 mA Ba(OH)2 and H2SO4 clear, colorless
10 mL 65 mA milky white precipitate forms
20 mL 31 mA more precipitate forms
30 mL 0 mA precipitate heavy and settles
40 mL 29 mA no added precipitate seen to form
50 mL 62 mA no change seen
Questions
1. Did you plot the data? yes or no
2. Did you label your graph axes? no or yes
3. Did you give your graph a title? no or yes
4. Does the Ba(OH)2 solution contain ions? yes or no
5. Does the H2SO4 solution contain ions? yes or no
6. Explain the data.
Is there any evidence that a reaction has occurred?
7. Does the conductivity increase or decrease?
8. Does the number of ions in solution increase, decrease, or remain constant?
9. What is the indicator of the number of ions in solution?
10. How does this evidence indicate that the reaction has occurred between ions?
11. The Ba(OH)2 dissociates as Ba+2 + 2 OH-. H2SO4 dissociates as 2 H+ + SO4-2.Write a balanced equation for this reaction.
12. When the conductivity is at a minimum, what must be true about the amount of Ba(OH)2?
13. Why does it not conduct at this low point?
14. Why does it conduct more before and after this minimum point?
The data obtained from the experiment shows a clear indication that a reaction has occurred between the H₂SO₄ and Ba(OH)₂ solutions. As the H₂SO₄ solution is added to the Ba(OH)₂ solution, the ammeter reading decreases indicating a decrease in conductivity.
The decrease in conductivity is due to the formation of an insoluble white precipitate, BaSO₄, as seen in observations. When no more H₂SO₄ is added, the ammeter reading stabilizes, indicating that the reaction has reached completion, as seen in observations e and f.
The formation of BaSO₄ precipitate indicates that the sulfate ion, SO₄²⁻, from H₂SO₄, has reacted with the barium ion, Ba²⁺, from Ba(OH)₂, forming an insoluble salt. This is a typical example of a precipitation reaction, where two aqueous solutions are mixed, resulting in the formation of an insoluble solid product.
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The question is inappropriate; The complete question is:
A chemistry student carried out an experiment with a conducting apparatus (ammeter) similar to the one below. This ammeter measures in milliamperes (mA). To 30 mL of the Ba(OH)2 solution, 10 mL portions of H2SO4 were added until a total of 50 mL of H2SO4 were used.
Explain the data. Is there any evidence that a reaction has occurred? How does this evidence indicate that the reaction has occurred between ions?
If an equal quantity of heat is added to equal masses of Copper and Water, estimate the final
temperature difference
The temperature of copper would rise by 263.8°C more than the temperature of water if we added the same amount of heat to equal masses of each substance.
What do you mean by specific heat capacity?Specific heat capacity is the amount of heat energy required to raise the temperature of one unit mass of a substance by one degree Celsius or Kelvin. To estimate the final temperature difference, we can use the specific heat capacity of each substance.
The specific heat capacity of copper is 0.385 J/g°C, while the specific heat capacity of water is 4.184 J/g°C. This means that water requires over ten times as much heat energy as copper to raise its temperature by one degree Celsius.
If we add an equal quantity of heat (in joules) to equal masses of copper and water, we can expect the temperature of copper to rise much more than the temperature of water. In fact, we can calculate the temperature difference using the following formula:
Q = mCΔT
where Q is the amount of heat added, m is the mass of the substance, C is its specific heat capacity, and ΔT is the change in temperature.
If we assume that we add the same amount of heat to equal masses of copper and water (let's say 100 grams each), then we can set up two equations using the specific heat capacities of each substance:
Q = 100 * 0.385 * ΔT (for copper)
Q = 100 * 4.184 * ΔT (for water)
Since Q is the same in both equations (we added the same amount of heat to each substance), we can set the two equations equal to each other and solve for ΔT:
100 * 0.385 * ΔT = 100 * 4.184 * ΔT
0.385 * ΔT = 4.184 * ΔT
3.799 * ΔT = Q (where Q is the amount of heat added)
ΔT = Q / 3.799
So, if we added 1000 joules of heat to 100 grams each of copper and water, we can expect the temperature difference between the two substances to be:
ΔT = 1000 / 3.799 = 263.8°C
This means that the temperature of copper would rise by 263.8°C more than the temperature of water if we added the same amount of heat to equal masses of each substance. However, it's important to note that this is a theoretical estimate, and in reality, there would be some loss of heat to the surroundings, which would affect the final temperature difference.
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