## Problem 4D.3

aphung1E
Posts: 101
Joined: Sat Aug 24, 2019 12:15 am

### Problem 4D.3

What equation(s) should be utilized to find the internal energy?
I have a feeling q=mcdeltat will be used.
The reaction of 1.40 g of carbon monoxide with excess water vapor to produce carbon dioxide and hydrogen gases in a bomb calorimeter causes the temperature of the calorimeter assembly to rise from 22.113 8C to 22.799 8C. The calorimeter assembly is known to have a total heat capacity (calorimeter constant) of 3.00 kJ?(8C)21. (a) Write a balanced equation for the reaction. (b) Calculate the internal energy change, DU, for the reaction of 1.00 mol CO(g).

Benjamin Feng 1B
Posts: 102
Joined: Sat Sep 07, 2019 12:19 am

### Re: Problem 4D.3

Since you are using a bomb calorimeter, volume is not changing so dU = q + w, where w = PdV. Since volume doesn't change, you can cancel out the w term and change in internal energy is just q. You still have to subtract the heat capacity times the change in pressure to account for the calorimeter.

Morgan Carrington 2H
Posts: 54
Joined: Wed Nov 14, 2018 12:22 am

### Re: Problem 4D.3

Benjamin Feng 1B wrote:Since you are using a bomb calorimeter, volume is not changing so dU = q + w, where w = PdV. Since volume doesn't change, you can cancel out the w term and change in internal energy is just q. You still have to subtract the heat capacity times the change in pressure to account for the calorimeter.

Why do you need to subtract the heat capacity times the change in pressure? What role does the calorimeter have on the reaction?