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When a 1.17 g sample of gaseous hydrogen bromide dissolves in 39.1 g of water in a coffee-cup calorimeter, the temperature rises from 20.00°C to 27.28°C.

Calculate [tex] \Delta H [/tex] in kJ/mol for HBr.

Answer :

Final answer:

The enthalpy change for the dissolution of hydrogen bromide in water is calculated to be approximately 82.75 kJ/mol HBr, which indicates it is an exothermic reaction.

Explanation:

To calculate the enthalpy change (H) for this chemistry question, you first need to determine the amount of heat transferred using the equation q = mcΔT, where m is the mass of water, c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature.

Hence, q = (39.1 g * 4.18 J/g°C * (27.28°C - 20°C)) = 1196.58 J.

Since 1KJ = 1000 J, the heat absorbed by the water is 1.19658 kJ.

You then calculate the moles of HBr by dividing the mass by the molar mass (1.17 g / 80.91 g/mol = 0.01446 mol).

Finally, you calculate the enthalpy change (in kJ/mol HBr) by dividing the heat absorbed by the moles of HBr (1.19658 kJ / 0.01446 mol = 82.75 kJ/mol).

Thus, the enthalpy change H is 82.75 kJ/mol HBr, which indicates this is an exothermic process, as the reaction released heat to the environment.

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