Question

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1. Given the standard enthalpy changes for the following two reactions:

(1) Ni(s) + Cl₂(g)--->NiCl₂(s)...... ΔH° = -305.3 kJ

(2) Fe(s) + Cl₂(g)-->FeCl₂(s)......ΔH° = -341.8 kJ

what is the standard enthalpy change for the reaction:

(3) Ni(s) + FeCl₂(s)--->NiCl₂(s) + Fe(s)......ΔH° = ?

____ kJ

2- When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter.

In the laboratory a general chemistry student finds that when 1.61 g of CaCl₂(s) are dissolved in 114.10 g of water, the temperature of the solution increases from 23.53 to 26.05 °C.

The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.77 J/°C.

Based on the student's observation, calculate the enthalpy of dissolution of CaCl₂(s) in kJ/mol.

Assume the specific heat of the solution is equal to the specific heat of water.

ΔH_dissolution = ____kJ/mol

3-

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 3.73 g of NH4ClO4(s) are dissolved in 114.20 g of water, the temperature of the solution drops from 25.53 to 23.15 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.63 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of NH4ClO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. ΔHdissolution = ____ kJ/mol

4-

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 20.03 g of BaBr2(s) are dissolved in 110.20 g of water, the temperature of the solution increases from 25.12 to 28.14 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.52 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of BaBr2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. ΔHdissolution = ____ kJ/mol

Answer 1

1st answer is