Solution Found!
An experimenter adds 970 J of heat to 1.75 mol of an ideal
Chapter 19, Problem 28E(choose chapter or problem)
An experimenter adds 970 J of heat to 1.75 mol of an ideal gas to heat it from \(10.0^{\circ} \mathrm{C}\) to \(25.0^{\circ} \mathrm{C}\) at constant pressure. The gas does + 223 J of work during the expansion.
(a) Calculate the change in internal energy of the gas.
(b) Calculate \(\gamma\) for the gas.
Questions & Answers
QUESTION:
An experimenter adds 970 J of heat to 1.75 mol of an ideal gas to heat it from \(10.0^{\circ} \mathrm{C}\) to \(25.0^{\circ} \mathrm{C}\) at constant pressure. The gas does + 223 J of work during the expansion.
(a) Calculate the change in internal energy of the gas.
(b) Calculate \(\gamma\) for the gas.
ANSWER:Solution 28E Step 1 of 7: a) Calculate the change in internal energy of the gas. In the given problem, we need to calculate change in internal energy for an ideal gas at constant pressure. Given data, Heat supplied, Q= 970 J Work done by ideal gas, W= 223 J Number of moles, n= 1.75 mol 0 Initial temperature, T = i0 c 0 Final temperature, T = 2f c Change in temperature, T = T T = 2f c i0 c = 15 c 0 0 Pressure, P=P = P f i To find, Change in internal energy, U =