textbook 4d.3

[Natalie Keung 1D]

4D.3 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 22.113C to 22.799C. The calorimeter assembly is known to have a total heat capacity (calorimeter constant) of 3.00kJ/C. (a) Write a balanced equation for the reaction. (b) Calculate the internal energy change for the reaction of 1 mol CO(g).

Hello! I understand how to calculate the q for the calorimeter and then dividing it by the moles of CO in 1.40g but I am confused as to what the information of 1 mol CO has to do with this problem. Can anyone explain why we disregard the 1 mol?
I have a feeling it is either additional information that isn't needed or it just means in the balanced equation? Unsure.

[Matthew Li 1B]

the q you calculate which is q= (22.799C-22.113C)*3 =2.058 is the heat released for each 1.4 g of carbon monoxide reacted. What b is asking is for is how much q can 1 mol of carbon monoxide produce. So u would then convert 1 mol of CO to grams which is 28g. Then you would divide -(28/1.4)*2.058 to see the what the heat released is, which would be negative as the system is losing heat.. And since there is no work done, the change of internal energy, delta U, equals q.