Given below are two statements: Statement I: For an ideal gas, heat capacity at constant volume is always greater than the heat capacity at constant pressure. Statement II: In a constant volume process, no work is produced and all the heat withdrawn goes into the chaotic motion and is reflected by a temperature increase of the ideal gas. In the light of the above statements, choose the correct answer from the options

Step-by-step solution

For an ideal gas, the relationship between heat capacity at constant pressure ( C_p ) and heat capacity at constant volume ( C_v ) is given by Mayer's relation: C_p - C_v = R Since the universal gas constant R is a positive value, C_p > C_v . Thus, Statement I is false. In a constant volume (isochoric) process, the change in volume V = 0 . Work done, W = P V = 0 . According to the first law of thermodynamics: U = q + W Since W = 0 , we get U = q_v . This means that in a constant volume process, no work is produced