1. In the laboratory a general chemistry student finds that when 2.47 g of CaBr2(s) are dissolved in 110.90 g of water, the temperature of the solution increases from 22.84 to 25.63 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.79 J/°C.
Based on the student’s observation, calculate the enthalpy of dissolution of CaBr2(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
ΔHdissolution = kJ/mol

2. In the laboratory a general chemistry student finds that when 1.99 g of CaBr2(s) are dissolved in 105.50 g of water, the temperature of the solution increases from 23.94 to 26.30 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.82 J/°C.
Based on the student’s observation, calculate the enthalpy of dissolution of CaBr2(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
ΔHdissolution = kJ/mol
3. Using standard heats of formation, calculate the standard enthalpy change for the following reaction.
CH4(g) + 2O2(g)CO2(g) + 2H2O(g)
ANSWER: kJ

4. Using standard heats of formation, calculate the standard enthalpy change for the following reaction.
NH4NO3(aq)N2O(g) + 2H2O(l)
5. A scientist measures the standard enthalpy change for the following reaction to be 2880.0 kJ :
6CO2(g) + 6 H2O(l)C6H12O6 + 6 O2(g)
Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(l) is kJ/mol.
6. A scientist measures the standard enthalpy change for the following reaction to be -1055.6 kJ :
2H2S(g) + 3 O2(g)2H2O(g) + 2 SO2(g)
Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is kJ/mol.
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