Suppose a 3000 c1113 container holds 7.0 g of nitrogen gas at a pressure of 200 kPa. The gas can be heated at constant pressure if a piston moves outward to let the gas expand as it's heated. Alternatively, the gas can be heated at constant volume if the piston is locked in place to prevent expansion. How does the heat required for one of these processes compare to the heat required for the other process? Part A What is the starting temperature of the gas? Express your answer in kelvins. You did not open hints for this part. ANSWER: Part 3 With the piston locked in place, the gas is heated until the pressure doubles. What is the final temperature? Express your answer in kelvins. You did not open hints for this part