## 8.51

Volume: $\Delta S = nR\ln \frac{V_{2}}{V_{1}}$
Temperature: $\Delta S = nC\ln \frac{T_{2}}{T_{1}}$

Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

### 8.51

Can someone please explain how to start/set up #53?
The reaction of 1.40g of carbon monoxide with excess water vapor to produce carbon dioxide and the hydrogen gasses in a bomb calorimeter causes the temperature of the calorimeter assembly to rise from 22.113 degrees Celsius to 22.700 degree celsius. The calorimeter assembly is known to have a total heat capacity of 3.00 kJ * (C)-1. (a) write a balanced equation for the reaction. (b) Calculate the internal energy change, DELTA U, for the reaction of 1.00 mol CO(g).

Cooper1C
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

### Re: 8.51

The first step is to balance the equation that they describe in the first sentence.
CO + H2O -> CO2 + H2

Then you know that the heat absorbed by the calorimeter is equal to the heat released by the reaction. qcal = -qrxn
And delta U = q because the reaction occurred in a bomb calorimeter (w = 0 because V is constant).