Name:
Per:
Date: _________________Row
Thermochemistry Review Worksheet
1.Definitions:
-Endothermic:
-Exothermic:
-Enthalpy:
-Law of Conservation of Energy
-Heat of Reaction:
-Heat of Fusion
-Specific Heat
2. Explain why water is used in a calorimeter? What unique properties does water have?
Calculations:
1. How many Joules of heat energy would be required to raise the temperature of
16.0g of lead from 25˚C to its melting point of 327˚C for a length of time long
enough to completely melt the lead. Given: The specific heat capacity of lead is
0.159J/gK and the molar enthalpy of fusion is 24.7J/g.
Specific heat is in Kelvin. Must convert C to Kelvin.
Q=mcΔT
Q=1460J
2. How much energy is absorbed by 300g of methanol, CH3OH, as it evaporates?
Given: The molar heat of vaporization is 35.3kJ/mol.
300 * (1/45.02) * (35.3/1) = 200 J (1 sigfig)
3. If 540g of water condenses on a car during a cool night, calculate the amount of
energy released to the air during this condensation. Given: The molar heat of
vaporization of water is 40.79kJ/mol.
540 * (1/18.02) * (40.79/1) = 1200kj 2 sig figs
4. Calculate the amount of energy that is needed to change 125g of ice at -25˚C to
water at 75˚C. Be sure to sketch a Phase Diagram of this process before beginning
the work. Given: Molar enthalpy of fusion is 6.009kJ/mol, molar enthalpy of
vaporization is 40.79kJ/mol, the specific heat of solid H2O is 2.1J/gK, the specific
heat of liquid H2O is 4.186J/gK, and the specific heat of gas H2O is 1.7J/gK.
125 * 2.1 * 100 = 26000kj
5. What is the molar enthalpy of the formation of 1mol H2SO4(l) given the following
information?
2H2(g) + O2(g)  2H2O(g)
ΔHrxn = -484kJ
2S(s) + 3O2(g)  2SO3(g)
ΔHrxn = -890kJ
H2(g) + 2O2(g) + S(s) H2SO4(l)
ΔHrxn = -814kJ
H2O(g) + SO3(g) H2SO4(l)
ΔHrxn = xkJ
115KJ
6. What is the molar enthalpy of the formation of 1mol C2H6 gas given the following
information?
C2H4(g) + 3O2(g)  2CO2(g) + 2H2O(l)
ΔHrxn = -1401kJ
2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l)
ΔHrxn = -3100kJ
2H2(g) + O2(g)  2H2O(l)
ΔHrxn = -572kJ
C2H4(g) + H2(g) C2H6(g)
ΔHrxn = xkJ
-137KJ
7. The reaction for the fermentation of glucose is …
C6H12O6 (aq)  2CO2(g) + 2C2H5OH(aq)
ΔHrxn = -67kJ
a. Is this reaction endothermic or exothermic?
b. Calculate the energy released when 250g of glucose C6H12O6 (aq) ferments.
250 * (1/180.07) * (-67/1) = -93KJ