A mixture of monoatomic and diatomic ideal gases has a specific heat ratio ($\gamma$) of 1.52. What is the ratio of the number of moles of the monoatomic gas to the number of moles of the diatomic gas?

First law of thermodynamics states that

The ratio of specific heats of a gas is $\gamma$ . The change in internal energy of one mole of the gas, when the volume changes from V to 2V at constant pressure p is

When gas in a vessel expands its internal energy decreases. The process involved is

In changing the state of thermodynamics from $A$ to $B$ state, the heat required is $Q$ and the work done by the system is W . The change in its internal energy is

For a certain gas, the ratio of specific heats is given to be $\gamma = 1.5.$ For this gas

First law of thermodynamics is based on

70 cal of heat is required to raise the temperature of 2 moles of an ideal gas from 30$^ \circ C$ to 35$^ \circ C$ while the pressure of the gas is kept constant. The amount of the heat required to raise the temperature of the same gas through the same temperature range at constant volume is (gas constant $R = 2\;{\rm{cal\;mo}}{{\rm{l}}^{ - 1}} - {{\rm{K}}^{ - 1}})$

If the heat 110 J is added to a gaseous system and it acquires internal energy of 40 J, then the amount of internal work done is

$100g$ of water is heated from ${30^0}C$ to ${50^0}C$. Ignoring the slight expansion of the water, the change in its internal energy is [specific heat of water is $4184\,\,J/kg/k$].

In the certain process, 400 cal of heat are supplied to a system and at the same time 105 J of mechanical work was done on the system. The increase in its internal energy is