Name ________________________
Calorimetry Worksheet-1
1. What is the number of calories needed to change the temperature of 50.0 g of water 15.0oC?
2. How many calories are needed to increase the temperature of 150.0 g water from 40.0oC to
65.0oC?
3. What temperature in oC is produced when 800.0 calories is absorbed by 100.0 g water?
4. How many grams of water can be heated from 20.0 oC to 75oC using 12500.0 Joules?
5. How many kilocalories are required to change the temperature of 300.0 grams of 0oC water to
40.0oC?
6. What is the final temperature after 80.0 calories is absorbed by 10.0g of water at 25.0oC?
Calorimetry Worksheet-2
1. The specific heat of aluminum is 0.900 J/goC.
a. How much energy is needed to raise the temperature of a 8.50 x 102g block of
aluminum from 22.8oC to 94.6oC?
b. What is the specific heat of aluminum in Joules per mole degree Celcius?
2. In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl are mixed.
Both solutions were originally at 24.6 oC. After the reaction, the temperature is 31.3 oC. What is
the enthalpy change for the neutralization of HCl by NaOH?
3. A swimming pool, 10.0 m by 4.0 m is filled to a depth of 3.0 m with water at a temperature of
20.2 oC. How much energy is required to raise the temperature of the water to 30.0 oC?
4. A 75.5 kg student at a temperature of 36.6 oC jumps into a hot tub containing 160,000 mL of
water on a cold winter’s day. The water, which is initially at a temperature of 39.856 oC, cools
down to a temperature of 38.652 oC and oddly enough, the student warms up to that same
temperature after a 35 minute soak. Calculate the specific heat of the student, assuming that no
heat is lost in the exchange.
Hess’s Law and Heats of Formation Worksheet
Use Hess's Law of Additivity to solve the following problems.
1. Calculate the enthalpy change for the following reaction :
2Al(s) + Fe2O3(s)
2Fe(s) + Al2O3(s)
Based upon the following information :
2Al(s) + 3/2O2 (g)
Al2O3(s)
2Fe(s) + 3/2O2(g)
Fe2O3(s)
∆H = -1669.8 kJ
∆H = +824.2 kJ
2. Calculate the enthalpy change for the formation of lead(IV) chloride by the reaction of lead
(II) chloride with chlorine.
3 PbCl2(s) + 3 Cl2(g)
3 PbCl4(l)
Use the following thermochemical equations :
Pb(s) + 2Cl2(g)
Pb(s) + Cl2
PbCl4(l)
∆H = -329.2 kJ
PbCl2(s)
∆H = +359.4 kJ
3. Determine the heat of reaction for this equation :
4 NO(g) + 2O2(g)
4 NO2(g)
Use the following reaction data :
1/2N2(g) + 1/2O2(g)
1/2N2(g) + O2(g)
NO(g)
NO2(g)
∆H = -90.4 kJ/mol
∆H = +33.6 kJ/mol
4. Calculate the heat of formation for ethane:
C2H4(g) + H2(g)
C2H6(g)
Based on the following information :
2H2(g) + O2(g)
2H2O(l)
C2H4(g) + 3O2(g)
2C2H6(g) + 7O2(g)
∆H = -572 kJ
2H2O(l) + 2CO2(g)
6H2O(l) + 4CO2(g)
∆H = -1401 kJ
∆H = +3100 kJ
7. Use the standard heat of formation table to calculate the change in enthalpy for each reaction.
(a) C2H4(g) + 3O2(g)
(b) CaCO3(s)
2CO2(g) + 2H2O(l)
CaO(s) + CO2(g)
(c) C6H6(l) + 9/2O2(g)
(d) 4NH3(g) + 5O2(g)
6CO(g) + 3H2O(l)
4NO(g) + 6H2O(g)
HEATS OF REACTION PROBLEMS WORKSHEET
Use the summation equation to calculate the heats of reaction of the following equations
(DO ALL WORK IN KILOJOULES!
2CH4(g) + O2(g)  2 CH3OH(g)
2C6H6(g) + 15O2(g)  12CO2(g) + 6H2O(g)
NH3(g) + HCl (g) 
2HI(g) + Br2(g)
NH4Cl(s)
 2BrI(g) +I2(g)
2HCl(g) + F2(g)  2HF(g) +Cl2(g)
2NaCl(s) +3O2(g)  2NaClO3(s)