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.

ΔH_dissolution =



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.

ΔH_dissolution =



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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