fanyattehedzg

2022-01-11

The enthalpy of combustion of benzoic acid $\left({C}_{6}{H}_{5}COOH\right)$ is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 1.9862 g of benzoic acid are burned in a calorimeter, the temperature rises from $21.84$ to ${25.67}^{\circ}C$ . What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2000 g.)

ambarakaq8

Beginner2022-01-12Added 31 answers

Step 1

Write a balanced thermochemical equation for the combustion of 1 mol of

Step 2

Calculate the molar mass of

Step 3

Calculate the heat of the reaction in joules:

1. Begin with the mass of the

2. Use the molar mass of

3. Use a thermostoichiometric ratio to convert moles of

4. Use a conversion factor to convert kilojoules to joules.

Step 4

Since heat transfers from the reaction to the calorimeter and water, then

0

Don Sumner

Skilled2023-05-29Added 184 answers

nick1337

Expert2023-05-29Added 777 answers

RizerMix

Expert2023-05-29Added 656 answers

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