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Textbook question 4D.3

Posted: Sat Feb 01, 2020 12:22 pm
by Paige Lee 1A
Could someone please explain how to get the correct answer for part b?
I keep getting 2.06kJ

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 degC to 22.799 degC. The calorimeter assembly is known to have a total heat capacity (calorimeter con- stant) of 3.00 kJ?

(b) Calculate the internal energy change, deltaU, for the reaction of 1.00 mol CO(g).

Re: Textbook question 4D.3

Posted: Sat Feb 01, 2020 1:28 pm
by Aman Sankineni 2L
The heat of the reaction is equal to the negative heat of the calorimeter because the calorimeter is gaining heat from the reaction. Hence to calculate heat gained by the calorimeter, we use C(delta T). The question asks for the internal energy change for the reaction of 1.00 mol CO. We are given 1.40 g of CO or 0.04998 mol CO. To find out the heat for 1 mol of CO, we divide the value of C(delta T) by 0.04998 mol CO to get -41.2 kJ/mol CO.