A cylinder containing 5.00 mol of nitrogen gas is at room temperature (300 K).If the volume of the gas container is held constant and the gas is heated,how much energy must be transferred by heat to the gas to increase its temperature by 100 K?

Question

Quizplus · Accepted Answer

The correct answer is A because the change in internal energy of an ideal gas is given by ΔU = (3/2)nRT, where n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. In this case, n = 5.00 mol, R = 8.314 J/mol·K, and ΔT = 100 K. Plugging these values into the equation, we get ΔU = (3/2)(5.00 mol)(8.314 J/mol·K)(100 K) = 1.04 * 10^4 J.

A Cylinder Containing 5