the phase of the copper product after the reaction in the copper cycle is listed below
1.the heating of Cu(OH)2 to form CuO i.e
Cu(OH)2 (s) ⇒ CuO(s) + H2O (l) which means the product of copper is in a solid phase after the reaction.
2.the addition of NaOH to Cu(NO3)2 to form Cu(OH)2 i.e
Cu(NO3)2 (aq) + NaOH (aq) ⇒Cu(OH)2 (s) + 2NaNO3 (aq) which means the product of copper is in the solid phase after the reaction.
3. the addition of HCL to CuO to form CuCl2 i.e
2 CuO(s) + 2 HCl(aq) ⇒ 2 CuCl2(aq) + H2O (aq) which means the product of copper is in the aqueous/liquid phase after the reaction.
4. the addition of Al to CuCl2 to form Cu i.e
Al(s) + CuCl2(aq) ⇒ AlCl3(aq) + Cu(s) which means the product of copper is in a solid phase after the reaction.
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What is the partial pressure (in atm) of co₂ at 468. 2 k in a 25. 0 l fuel combustion vessel if it contains 60. 0 grams co₂, 82. 1 g h₂o, and 7. 30 mol vaporized, yet uncombusted fuel?.
Answer:
2.09 atm
Explanation:
Given: Temperature of system. volume of system, and masses of component gasses.
In order to get the mole fraction which we will use later, convert the 60.0 g CO2 and 82.1 g H20 into moles and add the number of moles you got yo 7.30.
(60.0g CO2 / 44.01 g/mole) + (82.1g H20/18.02) + 7.30 moles unknown fuel
This should work out to about 13.22 moles total. Then, plug in your numbers to the ideal gas law (PV=nRT or P=nRT/V). This will result in the total pressure of the system. p=(13.22 moles)x(0.08206 l*ATM/moles *K)x(468.2)/25.0L. This equation results in a total of 20.3 atm. According to Daltons law of partial pressure, the mole fraction (moles of a gas over total moles) of a given gas times the total pressure of the container gives the partial pressure.
(1.36/13.22) * 20.3 atm=2.09 atm
Determine the total number of atoms for each chemical formula!!
Answer:
9 for the first one
19 for the second
20 for the third
13 for the fourth
9 for the fifth
you used naocl and nai to generate i2 in situ. you probably noted this visually by observing the formation of a red-brown color as iodine was produced. the redox equation is:
CIO- acts as the oxidizing agent from the given redox reaction
What is redox reaction?
Redox reactions are oxidation-reduction chemical reactions in which reactants undergo a change in their oxidation states. The term 'redox' is short form of reduction-oxidation.What are oxidizing agent?
An oxidizing agent is a chemical species that tends to oxidize other substances, i.e. cause an increase in the oxidation state of the substance by making it lose electrons. Common examples of oxidizing agents include halogens is, oxygen, and hydrogen peroxide (H2O2).It is the compound which oxidizes others and reduced itself.Oxidation ( reducing agent) - oxidation number increasesReduction ( oxidizing agent) - oxidation number decreasesThe oxidation state (number) of one of the element in oxidizing agent decreases.
The oxidation state of O atom = -2.
Oxidation state of Cl in ClO- :
x+(-2) = -1
x = +1
Oxidation state of Cl in Cl- = -1
Thus , the oxidation state of Cl decreases from +1 to -1 in the reaction.
So, the CIO- acts as the oxidizing agent.
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Note: The complete question is
You used NaOCl and Nal to generate I2 in situ. You probably noted this visually by observing the formation of a red-brown color as iodine was produced. The redox equation is:
2H+ (aq)+CIO- (aq)+2I− (aq)→Cl− (aq)+I2 (aq)+H2O(l)
What is acting as the oxidizing agent?
suppose at the end of the titration, the solution containing the ce3 ion is transferred to a volumetric flask and diluted to 500. ml. what is the concentration of ce3 in the diluted solution?m
The volume of the concentration of Ce3+ is x = 0.010548 mL
What is Cerium?
Cerium is a chemical element with symbol Ce and atomic number 58. Classified as a lanthanide, Cerium is a solid at room temperature.
The initial concentration of Ce4+ = 0.1758 mL
Volume of the volumetric flask = 30 mL
After , dilution the Ce4+ = 500mL
0.1758 x 30 = x x 500
x = 0.1758 x 30 / 500
x = 0.010548 mL
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we derive in class that the heat capacity at constant volume of an ideal monatomic gas is (3/2)kb per particle. what is the heat capacity at constant volume of 5 moles of an ideal monatomic gas is (in si units)? you have to be careful not to confuse between the heat capacity per mole, which has units j/mole/k, and the heat capacity of a sample of given size. if the amount of the material (i.e. sample size) is know, your answer for the heat capacity of the sample should be in j/k.
The heat capacity of the sample should be is 62.358J/K.
Calculation:-
Heat Capacity of 5 mole
5 x ( [tex]\frac{3}{2}[/tex] Kв x NA )
= 5 x ( [tex]\frac{3}{2}[/tex] R)
[tex]\frac{15}{2} R[/tex]
= [tex]\frac{15}{2}[/tex] x 8.3144
= 62.358J/K
Heat capacity is defined as the amount of heat energy required to raise the temperature of a given amount of matter by 1 degree Celsius. The heat capacity of a particular substance is a broad property as it depends on its size or quantity. The unit of heat capacity is Joule/Kelvin or Joule/Celsius.
Heat capacity or specific heat is the amount of heat required per unit mass to raise the temperature by 1°C. Specific heat capacity helps determine the processing temperature and amount of heat required for processing and helps distinguish between two polymer composites. The heat capacity of a substance is defined as the amount of thermal energy produced or released when the temperature of a unit mass of the substance changes by 1 °C.
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two flasks at the same temperature are joined by a glass tube with a stopcock. flask a is a 4.0 l flask containing n2 at 2.0 atm, while flask b is a 10.0 l flask containing co at 1.4 atm. what is the final pressure in the flasks after the stopcock is opened?
Final pressure in the flasks containing N2 and Co after the stopcock is opened is 1.57 atm
mole in flask A
Volume (V) = 4L
Pressure (P) = 2atm
Temperature (T) = STP = 273K
Gas constant (R) = 0.0821 atm.L/Kmol
Number of mole (n) =?
n = PV/RT
n = (2 × 4) / (0.0821 × 273)
n = 0.357 mole
mole in flask B
Volume (V) = 10L
Pressure (P) = 1.4atm
Temperature (T) = STP = 273K
Gas constant (R) = 0.0821 atm.L/Kmol
Number of mole (n) =?
n = PV/RT
n = (1.4 × 10) / (0.0821 × 273)
n = 0.625 mole
determining the final pressure
Total volume (V) = 4 + 10 = 14 L
Total mole (n) = 0.357 + 0.625 = 0.982
Temperature (T) = STP = 273 K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure (P) =?
P = nRT/V
P = (0.982 × 0.0821 x 273) / 14
P = 1.57 atm
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what is the empirical formula of a substance that contains 2.64 g of c, 0.444 g of h, and 3.52 g of o?
The empirical formula of the given substance is CH2O.
A molecular formula is the smallest integer ratio of the atoms of an element in a compound. Therefore, to find the empirical formula, first find the number of moles of each element and then find the molar ratio. Therefore, the mass of carbon is 2.64 g, the mass of hydrogen is 0.444 g, and the mass of oxygen is 3.52 g. So, with the help of this information and the product table in question, the molar mass of carbon is 12.1 g per molar mass of hydrogen is 1.8 g per molar mass of oxygen, i.e. 16 g per mole. Now, let's find the molar ratio of carbon, hydrogen, and oxygen. As we know, the number of Mohrs is equal to the given mass divided by the molar mass. From this we can find the molar ratio of carbon, hydrogen and oxygen, which is the molar ratio of carbon equal to the mass of carbon divided by the molar mass of carbon.
So solving gives 0.22, and similarly 0.44 for hydrogen. 0.22 for oxygen. Therefore, we can divide the above molar ratio by 0.22. Since this is the smallest number, it is the ratio of 0.22 divided by 0.22, the ratio of 0.44 divided by 0.22, and the ratio of 0.22 divided by 0.22. Therefore, this value equals 1. This value is equal to 1. That is, the molecular formula contains one carbon atom, two hydrogen atoms, and one oxygen atom.
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State the empirical formula for each of the following compounds:
a) C4H8
b) C₂H6O₂
c) N₂O5
d) Ba3(PO4)2
CH2 is the empirical formula.
The simplest whole number ratio of each kind of atom in the compound serves as its empirical formula. It may be calculated using information on the mass of each component in a compound or the composition's percentage.
The number of atoms that make up a single molecule of a substance is specified by both the empirical formula and the molecular formula. Even if it doesn't usually happen, the empirical formula and molecular formula of a molecule may one day match. You must first ascertain the relative masses of the individual components in order to construct the empirical formula. Either mass data given in grams or composition% can be used.
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Two carbon atoms (group 14) bond with two hydrogen atoms (group 1) to form acetylene (c2h2). How would each carbon atom in acetylene bond?.
11111111111111111111111111
We can conclude that each carbon atom in acetylene shares one pair of electrons with the hydrogen atom and three pairs with the other carbon atom.
A chemical bond is a long-lasting attraction between atoms or ions that allows molecules and crystals to form. Ionic bonds are formed by the electrostatic force between oppositely charged ions, whereas covalent bonds are formed by the sharing of electrons.
Each carbon atom in acetylene shares one pair of electrons with the hydrogen atom and three pairs with the other carbon atom.
The carbon atom contains four electrons. It requires four electrons to become stable in its outermost shell. Two carbon atoms covalently bond three pairs of electrons with each other in acetylene, and the remaining pair covalently bonds with two hydrogen atoms.
As a result of the carbon and hydrogen atoms becoming more stable, we can conclude that in acetylene, each carbon atom shares one pair of electrons with the hydrogen atom and three pairs with the other carbon atom.
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In lab we applied the conservation of energy to a system to allow us to equate the initial energy to the final energy. How does the initial energy become stored in the system?.
In lab we applied the conservation of energy to a system to allow us to equate the initial energy to the final energy. Here the initial energy become stored in the system. It is due the reason that:
The force of gravity does work on the mass when it is displaced some height when the pendulum is displaced by some angle theta.
Work done by the gravitational force is W = mgh , it is known as potential energy of the body.
When, body displaced some height then work done by the gravitational force store as energy in the system.
So, the force of gravity does work on the mass, when it is displaced some height .
What do you mean by force of gravity ?
“Every particle of matter in the universe attracts every other particle with a force that is directly proportional to the product of the masses of the particles and inversely proportional to the square of the distance between them.”
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Consider two 5 l chambers. In one, there are 5. 00 g o₂, and in the other there are 5. 00 g he. Which has the higher pressure at room temperature?.
The gas having higher pressure at room temperature, is P = 6.11 atm.
What is the ideal gas law?
The general gas equation, often known as the ideal gas law, is the equation of state for a hypothetical ideal gas. It has a number of limitations, but it provides a decent approximation of the behavior of numerous gases under various circumstances.
According to the ideal gas equation,
PV =nRT
For O₂,
Number of moles of oxygen gas = 5.00 g /32 g/mol = 0.156 moles
P =?
V = 5 L
n = 0.156 moles
T = 25 + 273 = 298 K
R = 0.082 atmLK-1mol-1
P = nRT/V
P = 0.156 moles × 0.082 atmLK-1mol-1 × 298 K/5 L
P = 0.76 atm
For He,
Number of moles of He = 5/4 g/mol = 1.25 moles
P =?
V = 5 L
n = 1.25 moles
T = 25 + 273 = 298 K
R = 0.082 atmLK-1mol-1
P = nRT/V
P =1.25 moles × 0.082 atmLK-1mol-1 × 298 K/5 L
P = 6.11 atm
Hence the gas having higher pressure at room temperature is He.
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2. write the pertinent hydrolysis reactions of the ions in the salt solutions and explain if the ph measured is reasonable for individual salts and discuss if the measured ph values agreed with the predictions.
The pertinent hydrolysis reactions of the ions in the salt solutions are as follows:
- For the Na+ ion, the hydrolysis reaction is:
Na+(aq) + H2O(l) → NaOH(aq) + H+(aq)- For the Cl- ion, the hydrolysis reaction is:
Cl-(aq) + H2O(l) → HCl(aq) + OH-(aq)- For the SO42- ion, the hydrolysis reaction is:
SO42-(aq) + 2H2O(l) → H2SO4(aq) + 2OH-(aq)What are the pH values measured for the individual salt solutions?The measured pH values for the individual salt solutions are as follows:
NaCl: 8.0CaSO4: 8.3MgCl2: 9.0The pH values measured for the individual salt solutions are reasonable. The measured pH values agree with the prediction.
The measured pH values agree with the predictions because the measured pH values are within the range of the expected pH values for each salt.
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Which transition of an electron in the hydrogen atom emits a photon with the smallest amount of energy?.
The transition n 2=∞ to n 1=2 emits radiation of the lowest wavelength. This transition corresponds to the maximum energy of emitted radiation.
What is emitted radiation?
When the excited electron transitions back to a lower electron orbital, emission takes place. The radiation that is emitted is known as luminescence. At energies equal to or lower than the energy corresponding to the absorbed radiation, luminescence can be seen. Following initial absorption, one of two pathways can lead to emission.
It is equal to the ionization energy and corresponds to the energy required when an electron is completely removed from the ground state of the hydrogen atom.
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calculate the number of moles of atoms in each of the following: 21. 3.01 x 1023 atoms of zinc 23. 1.806 x 1024 atoms of ba 22. 9.03 x 1023 atoms of s 24. 1.204 x 1024 atoms of na
The number of moles of atoms in each of the following is :
1) 0.5 mol
2) 2.9 mol
3) 1.49 mol
4) 1.9 mol
1) 3.01 × 10²³ atoms of zinc
3.01 × 10²³ atoms of zinc = (3.01 × 10²³) / (6.022 × 10²³) moles
= 0.5 mol
2) 1.806 × 10²⁴ atoms of Ba
1.806 × 10²⁴ atoms of Ba = (1.806 × 10²⁴ ) / (6.022 × 10²³) moles
= 2.9 mol
3) 9.03 × 10²³ atoms of S
9.03 × 10²³ atoms of S = 9.03 × 10²³ / (6.022 × 10²³) moles
= 1.49 mol
4) 1.204 × 10²⁴ atoms of Na
1.204 × 10²⁴ atoms of Na = 1.204 × 10²⁴ / (6.022 × 10²³) moles
= 1.9 mol
Thus, The number of moles of atoms in each of the following is :
1) 0.5 mol
2) 2.9 mol
3) 1.49 mol
4) 1.9 mol
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Which is an example of a chemical change?
O water evaporating from a puddle
O cloth tearing when pulled
O wood forming sawdust when cut
O bread baking in an oven
Answer: bread baking in a oven and water evaporating in a puddle
Explanation:
why is it necessary to exclude water in each stage of the production of a product with the grignard reaction. be specific. give a chemical equation to illlustrate
The water reacts with the Grignard reagent and destroys it. So it is necessary to exclude water in each stage of the production of a product with the Grignard reaction.
Consequently, water ought to be excluded from the reaction as plenty as possible i.e. by means of the usage of anhydrous solvents, etc. c. The addition of hydrochloric acid is essential to quench the leftover Grignard reagent and to transform the magnesium alcoholate into the alcohol.
Water or alcohols could protonate and for that reason destroy the Grignard reagent, due to the fact the Grignard carbon is tremendously nucleophilic. this would form a hydrocarbon.
Grignard reagents react swiftly with acidic hydrogen atoms in molecules consisting of alcohol and water. whilst a Grignard reagent reacts with water, a proton replaces the halogen, and the product is an alkane. The Grignard reagent, therefore, affords a pathway for converting a haloalkane to an alkane in steps.
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the density of solid cr is 7.15 g/cm3. how many atoms are present per cubic centimeter (cm3) of cr? cr atoms: atoms/cm3
One cubic centimeter of 7.15 g/cm³ will contain 9.2 x 10²² Cr atoms.
The density of Cr is 7.15 g/cm³.
It means, one cm³ contains 7.15 grams of Cr.
We know moles are given by,
n = mass/molar mass
n = number of atom/Avogadro number
Molar mass of Cr is 51 g/mol.
So, the number of atoms per cubic centimeter can be found as,
7.15/51 = Number of atom/6.603 x 10²³
Number of atoms = 9.2 x 10²²
So, one cubic centimeter will contain 9.2 x 10²² atoms of Cr.
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Select the set of reactants that will form a precipitate upon mixing.
Li2S(aq) + NiCl2(aq)
Na3PO4(aq) + H2SO4(aq)
NaClO4(aq) + Fe(NO3)2(aq)
NaCl(aq) + KBr(aq)
BaCl2(aq) + LiOH(aq)
A precipitate can be produced by the combination of lithium sulfide and nickel II chloride.
What is a precipitate?The term precipitate has to do with a solid product that is obtained from an aqueous phase reaction. It is important to know that in this kind of reaction, we have two aqueous phase reactants but they combine to give an insoluble product.
In this case we have to look at the possible products of each of the reactants as we have them in the question. The question that we must ask ourselves is; which of these aqueous reactants can produce a solid product?
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How does potential energy relate to bond forming?
What evidence did you ee that indicated the liquid from copper (11) ulfate or Tagu rate wa waterr
Evidence did you see that indicated the liquid from copper II sulfate pentahydrate was water is color change to adding water to anhydrous copper II sulfate
Copper II sulphate also known as copper sulphate is an inorganic compound with the chemical formula CuSO₄ and when liquid from copper II sulfate pentahydrate was water then the color change from pale blue to white and change back to blue when water is added and the color change on adding water to anhydrous copper II sulphate has been used as test for the presence of water in a liquid
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Please help me with the problem
The following are :
(a) compound
(b) compound
(c) mixture
(d) mixture
In first one is red atom is bonded with one white atom and all the given are the same so this is an compound. in the second one the one red atom bonded with two white atom and all are the same this means this is also compound. the third one is one is bonded with same atom but it also have another atom bonded with same atom so this is a mixture. this kis exact same case in the fourth one there mixture.
Thus, The following are :
(a) compound
(b) compound
(c) mixture
(d) mixture
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A solution is prepared by dissolving 15. 0 g of nh3 in 250. 0 g of water. The density of the resulting solution is 0. 974 g/ml. What is the mole fraction of nh3 in the solution?.
Mole fraction of nh3 in the solution is 11.33%.
What is mole?
The International System of Units uses the mole (symbol: mol) as the unit of substance amount (SI). How so many elementary entities of a particular substance are present in an object or sample is determined by the quantity of that substance. There are precisely 6.02214076×10^23 elementary entities in a mole.
NH3(g) + H2O(l) = NH4OH (aq)
The molar mass of NH3 is 17.031 g/mol.
The NH3:NH4OH mole ratio is 1: 1.
Mol of NH3 = 15 g/(17.031 g/mol) = 0.88 mol, which produces (1/1) x 0.88 mol of NH4OH = 0.88 mol of NH4OH/250 g of water.
The mass of the solution is calculated as 15g + 250 g = 265 g.
Given that the density of NH4OH is 0.974 g/mL, the resulting solution contains 0.88 mol of NH4OH/265 g: 0.974 g/mL or 0.88 mol/272.0739mL.
Then, mol of NH4OH in 100mL solution = (100mL/272.0739mL) x 0.88 mol = 0.3234 mol of NH4OH/100mL solution...
……. [A]
The molar mass of NH4OH is 35.04 g/mol.
As a result, the mass of NH4OH = 0.3234 mol x 35.04 g/mol = 11.33 g of NH4OH/100mL or 11.33% (m/v).
As stated in [A], one mol of NH4OH equals 0.3234mol/100mL solution or (1000mL/100mL) x 0.3234 mol equals 3.234 mol NH4OH/L or 3.234 M.
Because NH4OH is a monoprotic base, molarity equals normality, so the resulting solution's normality = 3.234 N rounded up to 3.23 N.
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In a lewis structure involving bromine and chlorine, if a central bromine atom has two lone pairs, how many chlorine atoms must be present?.
Learn Lewis dot structure and lone pair.
What is lewis structure?
The valence shell electrons of a molecule are depicted in a highly condensed manner in a Lewis structure. It serves as a visual representation of the electron arrangements around specific atoms in molecules. Electrons are represented as "dots" or "lines" when two atoms are bonded together.
What is lone pair?
Valence electron pairs known as lone pairs are those that are exclusive to one atom. They are not involved in the synthesis of covalent bonds. An example is the two lone pairs on the oxygen atom in the water molecule. Another illustration is the lone pair on the nitrogen atom of the ammonia molecule.
Four of the seven valence electrons in bromine are occupied if there are two lone pairs. Thus, three chlorine atoms can form covalent connections with the remaining three.
Therefore, three chlorine atoms can form covalent connections with the remaining three.
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Which product uses materials gained from smelting iron ore?
Responses
coal
coal
steel
steel
uranium
uranium
oil
oil
Answer: The Answer is Steel
Explanation:
when comparing hclo and hbro , hclo is a acid than hbro .target 1 of 4 when comparing h2so4 and h2so3 , h2so4 is a acid than h2so3 .target 2 of 4 when comparing ccl3cooh and ch3cooh , ccl3cooh is a acid than ch3cooh .target 3 of 4 when comparing hclo2 and hclo , hclo2 is a acid than hclo .
When comparing HClO and HBrO, HClO is a stronger acid than HBrO because it has more electronegative atoms.
When comparing H₂SO₄ and H₂SO₃, H₂SO₄ is a stronger acid because it has more oxygen atoms. As we know that the higher number of oxygen atoms in oxyacids increases the acidic strength of the acid.
When comparing HClO₂ and HClO, HClO₂ is a stronger acid because it has more oxygen atoms. As we know that the higher number of oxygen atoms in oxyacids, Increases the acidic strength of the acid.
When comparing HCLO and HBrO, HClO is a stronger acid because it has more electronegative atoms. As we know that the electronegativity of chlorine is higher than that of bromine.
When comparing CCl₃COOH and CH₃COOH, CCl₃COOH is a stronger acid because it has more electronegative atoms. As we know that the electronegativity of chlorine is higher than that of oxygen.
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___________ is the property of a material to not change shape when squeezed
Elasticity is the property of a material to not change shape when squeezed.
Elasticity of the material is the property of a material that regain its shape after the material is stretched or compressed. This is an elastic force. whenever the material is compressed or we stretched it then the force called elastic force act on it. when the material is more stretched or more compressed than the more elastic force act on it. when we stretched the material its shape changes and when we leave it it will regain its shape.
Thus, Elasticity is the property of a material to not change shape when squeezed.
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Calculate the amount of heat that must be absorbed by 10. 0 g of ice at –20°c to convert it to liquid water at 60. 0°c. Given: specific heat (ice) = 2. 1 j/g·°c; specific heat (water) = 4. 18 j/g·°c; δhfus = 6. 0 kj/mol.
The amount of heat to absorb is 6261 J
The heat capacity is the amount of heat expressed usually in Joules or calories needed to change the system by 1 degree Celsius
Here the calculation for heat is
Heat required to raise the temprature of ice form -20°C to 0°C
Then the formula for specific heat is used to calculate the amount of heat
Q = c×m×ΔT
Where Q = heat exchanged by a body
m = mass of the body
c = specific heat
ΔT = change in temprature
Then the given data is
m = 10g
Specific heat of the ice = 2.1
ΔT = 0°C - (-20°C) = 20°C
Then substituting the value
Q = 10g× 2.1× 20°C
Q = 420 J
Heat required to convert 0°C ice to 0°C water
The heat Q necessary to melt a substances depend on its mass m and this called latent heat of fusion of each substances
Q = m×ΔH fusion
Heat required to raise the temprature of water from 0°C to 60°C
m = 10g
Specific heat of water = 4.18
ΔT = 60°C -(- 0°C) = 60°C
Then substituting
Q = 10g×4.18×60°C
Q = 2508 J
Then Q total = 420J+3333J+2508J
Q total = 6261 J
The amount of heat to absorb is 6261 J
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air is composed of approximately 78% n2, 21% o2 and 1% percent other gases. calculate the density of he at stp and explain why a closed balloon filled with he rises in air
Air is composed of approximately 78% N₂, 21% O₂, and 1% percent other gases, the density of He at stp will be 0.1637 g/L
At standard, temperature, and pressure (STP) the values are:
Pressure (P) = 1 atm
Temperature (T) = 25 °C or 298.15 K
Density of helium (He) = ?
To calculate the density of He, we will use the modified form of ideal gas law as:
PV = nRT
n = number of moles
n = m / M
Put the value of n in ideal gas law
PV = mRT / M
m / V = PM / RT
Where m = mass
M = molarity
V = volume
P = pressure
T = absolute temperature
R = universal constant of gasses (value = 0.082 atm.L / mol.K)
As we know that:
Density = m / V
Put density in place of m / V, the above equation will be:
Density = PM / RT
Put the values:
Density of Helium (He) = (1 atm) × (4.0026 g/mol) ÷ (0.082 atm.L/mol.K)(298.15 K)
Density of Helium (He) = 0.1637 g/L
A ballon filled with He rises because the density of He is lower than air.
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How many atoms of hydrogen in the product side of the balanced equation? fe + h2o ---> feo + h2.
Two atoms of Hydrogen should be on the product side of the balanced equation.
Balancing the chemical equation is the branch of chemistry which helps us in balancing the atoms that are present on both the reactants and on the product sides.
Once all the individual elements are balanced, the total number of atoms of each element on the reactant and product side are compared once again. To make sure that there are no inequalities, then the chemical equation is said to be balanced.
In the above given reactions we can see that in the reactant side there are 2 atoms of hydrogen in water molecule and in the product .
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Glycerol (molar mass= 92.09g/mol) has an enthalpy of combustion of -1654 kJ/mol. What mass of glycerol is needed to raise the temp of 50.0g water by 30.0°C?
Glycerol (molar mass= 92.09g/mol) has an enthalpy of combustion of -1654 kJ/mol. The mass of glycerol is needed is
Q water = mc ΔT
= 500 × 4.184 × ( 100 - 20)
= 167.36 kJ
Q glycerol = 167360 J = n ΔH
167360 = n × ( 1654)
n = 0.101 mol
mass = moles × molar mass
= 0.101 × 92.09
= 9.3 g
Thus, Glycerol (molar mass= 92.09g/mol) has an enthalpy of combustion of -1654 kJ/mol. mass of glycerol is needed to raise the temp of 500 g water from 20 °C to 100 °C is 9.3 g.
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