I can’t solve the questions from the first morning of the professional exam after 10 years

What is the heat (in kJ) required to raise 3.1 mol of carbon dioxide from 400 K to 1100 K? It is known that the average heat capacity of carbon dioxide between 298 and 400 K is Cp1-=39.23 J/(mol•K); at 400 K, its true heat capacity is Cp1=41.05 kJ/(mol•K), and at 1100 K, it is Cp2=55.65 kJ/(mol•K). A. 30.7 B. 34.9 D. 37.74

I spent ages trying, but I still haven’t mastered the trick of sending photos quickly:L

This post was last edited by zshiwei2008 on 2016-8-5 17:30. This question is question number 3 from the morning of the first day of 2010; the original question reads as follows: What is the amount of heat (in kJ) required to raise 1 mole of carbon dioxide from 400 K to 1100 K? It is known that the average heat capacity of carbon dioxide between 298 and 400 K is Cp_avg = 39.23 J/(mol·K); at 400 K, its true heat capacity is Cp1 = 41.05 kJ/(mol·K), and at 1100 K, it is Cp2 = 55.65 kJ/(mol·K). A. 30.7 B. 34.9 C. 44.8 D. 37.74 This question primarily tests the difference between true heat capacity and average heat capacity. As we know, in the formula Q = mCp(t2 – t1), Cp refers to the average heat capacity. It is said online that the coefficient method can be used: Cp = A + BT + CT²; by substituting the values of Cp at the three temperatures, values for A, B, and C can be determined, and after integration, the answer can be obtained. It’s quite troublesome, and it seems that the unit for specific heat capacity is incorrect. However, since this is a multiple-choice question based on knowledge, no calculation is required; Cp should be taken as the arithmetic average of the true specific heat capacities. The answer is fairly close to option B, so guessing might work as well.

For question 3 on the morning exam, I thought it couldn’t possibly be that complicated; either it was a guess by the person above, or some parts of this question were misstated