Embibe Experts Solutions for Exercise 1: EXERCISE

A given mass of ideal gas changes its state from $A$ to $B$ along three different paths $1,2$ and $3.$ If $Q_1,Q_2$ and $Q_3$ be the heat supplied to the gas along respective paths then

For a given amount of ideal gas, if $A$ be the slope of $P~V$ curve for its isothermal process and $B$ be the slope of $P~V$ curve for its adiabatic process then $\gamma \left(=\frac{C_p}{C_v}\right)$ equals

Two moles of an ideal gas undergoes adiabatic process and changes its state from $(P_1, V_1, T_1)$ to $(P_2, V_2, T_2)$. The change in internal energy of the gas will be

At a constant pressure, a given amount of ideal diatomic gas expands under normal condition. The heat supplied to the gas is $350 \mathrm{J}.$ Then

A mixture of gases contains $4$ moles of oxygen and $2$ moles of argon at absolute temperature $T.$ The total internal energy of this system (neglecting vibrations) is $[R=$ universal gas constant ]

Two samples A and B of a gas initially at the same temperature and pressure, are compressed from the volume, $V$ to $\frac{V}{2}$ ($A$ isothermally and, $B$ adiabatically). The final pressure

A gas is suddenly compressed to $\frac{1}{4}$ th of its original volume. Rise in temperature of the gas if initial temperature is $27°\mathrm{C}$, will be (given $\gamma =1.5).$

An ideal gas is heated at constant pressure and absorbs$\text{'}Q\text{'}$ amount of heat. If the ratio $\frac{C_p}{C_v}=\gamma ,$ then