Name:
_____________________________________
Period ________________________
Calorimetry
1.
A BOMB calorimeter has a heat capacity of 40.00 kJ/C. Complete combustion of 1.00 g of hydrogen (H2(g)) in
this calorimeter causes the temperature to increase by 3.54C. Calculate the molar enthalpy of combustion of
hydrogen from this evidence. Write the balanced chemical equation with the energy term.
2.
A reference gives the molar enthalpy of combustion for methane as -803 kJ/mol. What minimum mass of
methane (CH4(g)) must be burned to warm 4.00 L of water from 22.4C to 87.6C, assuming no heat losses to the
surroundings?
3.
Combustion of 3.50 g of ethanol (C2H5OH(l)) in a BOMB calorimeter with a heat capacity of 15.2 kJ/C causes a
temperature increase from 19.88C to 26.18C. Find the molar enthalpy of combustion for ethanol from this
evidence. Write the balanced chemical equation with the energy term.
4.
Find the temperature increase expected from 1.00 L of water when it absorbs all of the energy from the
combustion of 1.00 g of acetylene (C2H2(g)). The molar enthalpy of combustion of acetylene is -1.29 MJ/mol.
Write the balanced chemical equation with the energy term.
5.
A student mixed 100.0 mL of 1.50 mol/L of sulfuric acid with 200.0 mL of 1.50 mol/L sodium hydroxide. Both
solutions were at 19.67C initially and the highest temperature reached by the reaction mixture was 34.06C.
Calculate the molar enthalpy of neutralization for sulfuric acid. (This is a difficult problem, refer to your
notes!!) Write the complete balanced chemical equation for the reaction including the energy term!!!