I have two problems actually: Problem 1 1. The problem statement, all variables and given/known data What mass of carbon dioxide can be produced at a temperature of 1500 *C and an atmospheric pressure of 92.5 kPa, if 15.5 L of acetylene gas is burned at STP? 2. Relevant equations PV = nRT P1V1/T1 = P2V2/T2 3. The attempt at a solution First, I found the amount of moles of acetylene gas, using the ideal gas law, PV = nRT nacetylene = 0.692 mol Then, I used a mole ratio according to the equation to find the moles of carbon dioxide gas: 2C2H2 + 5O2 → 2H2O + 4CO2 And 1.384 mol of carbon dioxide gas should be produced, multiplied by its molar mass of 32, I got 60.9 g. What confuses me is the 1500 *C and 92.5 kPa. The question was out of four marks and my solution seems worth that many marks. However, when I asked about it, my chemistry teacher sternly implied that the 1500 C and 92.5 kPa is relevant. This is my alternative solution, that gives the same answer, requires more work but does account for both the above values: Used mole ratio to go from 15.5 L acetylene to 31 L carbon dioxide gas. Converted from STP (31 L) to the given conditions, which satisfy the ideal conditions for an ideal gas that I found online (which was not in the course) that says that gases are "more" ideal at high temperature and low pressure: 92.5 kPa < STP, 1500 C > STP. I now had 220.5 L volume at the temperature and pressure given and used the ideal gas law to solve, and got the same answer: 92.5 kPa * 220.5 L/ 8.31 J * mol-1 * K-1 * 1773 K = 1.38 mol. I got zero on the question. Thanks in advance for ANY AND ALL input! :) I think the second one is slightly more appropriate, but both directions give the same answer, and considering that I barely had time to finish the test, the first approach seemed more practical.