Molar heat of vaporization is defined as the heat absorbed by one mole of substance to convert from liquid to gas.
<h3>How do you calculate the heat of vaporization?</h3>
The formula used to calculate the heat of vaporization is:
Where,
Q = Amount of Heat
n = number of moles of a substance
molar enthalpy of fusion
Now, to calculate the moles of methane:
Moles = 3.425 mol
Now, 1 mol of methane absorbs = 8.53 KJ
3.425 mol of methane absorbs = 
Thus, the energy is absorbed till the methane vaporizes at its boiling point is 29.1 KJ.
Learn more about <u>vaporization </u>here:
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Answer:
Mass = 0.697 g
Explanation:
Given data:
Volume of hydrogen = 1.36 L
Mass of ammonia produced = ?
Temperature = standard = 273.15 K
Pressure = standard = 1 atm
Solution:
Chemical equation:
3H₂ + N₂ → 2NH₃
First of all we will calculate the number of moles of hydrogen:
PV = nRT
R = general gas constant = 0.0821 atm.L/mol.K
1atm ×1.36 L = n × 0.0821 atm.L/mol.K × 273.15 K
1.36 atm.L = n × 22.43 atm.L/mol
n = 1.36 atm.L / 22.43 atm.L/mol
n = 0.061 mol
Now we will compare the moles of hydrogen and ammonia:
H₂ : NH₃
3 : 2
0.061 : 2/3×0.061 = 0.041
Mass of ammonia:
Mass = number of moles × molar mass
Mass = 0.041 mol × 17 g/mol
Mass = 0.697 g
Answer:
The solution becomes diluted.
Explanation:
When you add water to a solution, the number of moles of the solvent stays the same while the volume increases. Therefore, the molarity decreases.
Hope this helps!
