Name_________________________________
Section______
XXX_______
AP CHEMISTRY PROBLEM SET 3
3-1
The decomposition of solid ZnCO3 into solid ZnO and carbon dioxide
requires the addition of 71.5 kJ of heat per mole of zinc carbonate.
(a) Write a balanced equation for this reaction including states of matter.
(b) Calculate the volume of carbon dioxide produced by the decomposition
of XXX g of zinc carbonate if the reaction is carried out in a container
at exactly one atmosphere pressure and 25.0˚C.
(c) How many kilojoules of work are done by the generation of carbon
dioxide gas?
(d) How much heat was absorbed by the decomposition of the ZnCO3?
(e) What is the total change in energy for the reaction?
3-2
(a) Calculate the enthalpy change (∆H) in kJ for the following reaction:
2C(s) + H2(g)  C2H2(g)
Given the following information:
C2H2 (g) + 5/2 O2(g)  2CO2(g) + H2O(l) ∆Hrxn = -1299.6 kJ
C(s) + O2(g)  CO2(g)
∆Hrxn = - 393.5 kJ
H2(g) + ½ O2(g)  H2O(l)
∆Hrxn = - 285.8 kJ
(b) How much heat (in kJ) is absorbed or released when XX.X g of
carbon is consumed in this reaction??
3-3
When a 2.45 g piece of an unknown substance absorbs XXX.0 J of heat
the temperature increases from 25.00 °C to 163.50 °C. Calculate the
specific heat capacity of the material.
3-4
The heat of neutralization of HCl by NaOH is ΔH˚rxn= -56.2 kJ/mol.
(a) Write a complete, balanced, thermochemical equation for this reaction.
(b) How much heat is released when XXX.0 mL of 1.750 M HCl is mixed
with (1000.0 – XXX.0) mL of 0.667 M NaOH?
3-5
(a) A sample of ethanol, C2H5OH, weighing 0.XXX0 g is combusted
in a bomb calorimeter, resulting in a 24.50 °C rise in temperature.
A sample of propanol, C3H7OH, weighing 0.5000g is burned in the
same calorimeter, resulting in a 45.67 °C rise in temperature. The
heat of combustion of ethanol is 1368 kJ/mole.
(b) Calculate the amount of heat released when the sample of ethanol
burns.
(c) Calculate the heat capacity of the calorimeter.
(d) Calculate the molar heat of combustion of propanol.