Question

For constant volume processes the heat capacity of gas A is greater than the heat capacity of gas B. We conclude that when they both absorb the same energy as heat at constant volume:
A. the temperature of A increases more than the temperature of B
B. the temperature of B increases more than the temperature of A
C. the internal energy of A increases more than the internal energy of B
D. the internal energy of B increases more than the internal energy of A
E. A does more positive work than B

Answer 1

Answer:

B). the temperature of B increases more than the temperature of A

Explanation:

For constant volume process, relation between molar heat capacity and temperature is given by,

$\Delta Q = mC_v \Delta T$

where, ΔQ is the amount of heat required

              m is the mass of the gas

              $C_v$ is heat capacity at constant volume

              ΔT is the change in temperature.

For a constant energy ΔQ,

$C_v=\frac{1}{\Delta T}$

Given, $(C_v)_A>(C_v)_B$

∴     $(\Delta T)_A < (\Delta T)_B$

Thus the temperature of gas B increases more than the temperature of gas A.