By heating 2 mol of nitrogen gas in a frictionless piston-cylinder, the gas expands at a constant pres- sure of 1 bar from an initial volume of 0.02 m5 to a final volume of 0.05 m5. the gas temperature correspondingly increases from 300 to 500 k. assuming nitrogen is an ideal gas with a molar heat capacity c ^r (where r is the gas constant), find the amount of heat added and work derived from the gas expansion.

Ithink the answer is d.

Use the universal gas law formula: pv = nrt now, the key word in this problem is stp, so at stp, temperature will always be 0 degrees celsius and pressure will always be 1.0 atm or 760 torr. given something is at stp, we already know the two variables pressure and temperature. the other thing we can find with the given information is moles. to find moles, just divide grams by molar mass of the element. 16.0g / 2(16.00)g/mol = 0.5 moles plug the values in to the equation pv = nrt (1.0 atm)( x ) = (0.5 )(0+273=273k) the r value is just a constant for when we use atm, liters, moles and kelvin. i'm assuming you want your answer in liters, but if you dont just move the decimal 3 to the right in your final answer. so when plugging these numbers in to your calculator and trying to find x, you get 11.20665 liters using significant figures the answer is 11.2 liters