Suppose a 3000 cm3 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? V Part D V Returning to the starting conditions, the gas is heated but the piston is allowed to move in a way that keeps the pressure constant. What is the final temperature if the gas is heated until the volume doubles? Express your answer in kelvins. D View Available Hint(s) Tf=580K Previous Answers v Correct Correct answer is shown. Your answer 577 K was either rounded differently or used a different number of significant figures than required for this part. Doubling the volume at constant pressure doubles the temperature. Note that this is the same as the temperature you found in Part B, so both processes increase the temperature by the same amount. V PartF The constant-volume and constant-pressure processes both heated the gas to the same final temperature and thus both processes have the same AEth, but the constant- pressure process requires more heat. Why? Because work is done during the constant- pressure process but not during the constant-volume process. Recall that work is done on a gas only if the volume changes, meaning that a force acts on a piston as it moves in or out. How much work is done on the gas in the constant-pressure process of Part D? V View Available Hint(s) v Hint 1. How to approach the problem In general, the work done on a gas is W = Li pdV. If the pressure is constant and is taken outside the integral, then the work done during a constant-pressure process is W = pAV. E \"A 4 a o :2 m Previous Answers Ft_equest Answer X Incorrect; Try Again; 7 attempts remaining Check your signs