Work done by a sample of an ideal gas in a process A is double the work done in another process B. The temperature rises through the same amount in the two processes. If C_A and C_B be the molar heat capacities for the two processes.

For a solid with a small expansion coefficient,

The value of C_P – C_V is 1.00 R for a gas sample in state A and is 1.08R in state B. Let P_A, P_B denote the pressures and T_A, and T_B denote the temperatures of the states A and B respectively. Most likely

Let C_V and C_P denote the molar heat capacities of an ideal gas at constant volume and constant pressure respectively. Which of the following is a universal constant?

70 calories of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30°C to 35°C. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is

The molar heat capacity for the process shown in the figure is

The molar heat capacity for the process shown in the figure is

In an isothermal process on an ideal gas, the pressure increases by 0.5%. The volume decreases by about

In an adiabatic process on gas with γ = 1.4, the pressure is increased by 0.5%. The volume decreases by about

Two samples A and B are initially kept in the same state. Sample A is expanded through an adiabatic process and sample B through an isothermal process. The final volumes of the samples are the same. The final pressures in A and B are p_A and P_B respectively.

Let T_a and T_b be the final temperatures of the samples A and B respectively in the previous question.

Let ΔW_a and ΔW_b be the work done by the systems A and B respectively in the previous question.

The molar heat capacity of oxygen gas at STP is nearly 2.5R. As the temperature is increased, it gradually increases and approaches 3.5R. The most appropriate reason for this behaviour is that at high temperatures.