Specific Heat Capacity

Which one of the following material will expand maximum if the same amount of heat energy is given to them?

How much heat energy is necessary to raise the temperature of $2 \mathrm{kg}$ of ice from $-20°\mathrm{C}$ to steam at $120°\mathrm{C}$?

The volume of $n$ moles of an ideal gas with degree of freedom $f$ is varied according to the law $V=\frac{a}{T}$ where $a$ is a constant. The molar specific heat of the gas at constant pressure is

Two identical systems, with heat capacity at constant volume that varies as $C_v=b{T}^3$ (where $b$ is a constant) are thermally isolated. Initially, one system is at a temperature $100\mathrm{ }\mathrm{K}$ and the other is at $200 \mathrm{K}$ . The systems are then brought to thermal contact and the combined system is allowed to reach thermal equilibrium. The final temperature (in $\mathrm{K}$ ) of the combined system is $\alpha$. Write the value of $\left[\alpha \right],$ where $\alpha$ is the greatest integer function.

During an adiabatic process, the pressure of a gas is found to be proportional to the cube of its absolute temperature. The ratio $\frac{C_{\mathrm{P}}}{C_{\mathrm{V}}}$  for the gas is $\frac{x}{2}$. Find $x$.

The piston is massless and the spring is ideal and initially streched the piston cylinder arrangement encloses an ideal gas. If the gas is heated quasistatically the $PV$ graph.

Figure shows a long fixed container which has two freely movable (without friction) pistons. The container and pistons are made of a thermally conducting material that allows very slow transfer of heat. First compartment of container is filled with $2$ moles of an ideal monoatomic gas at $200 \mathrm{K}$ and the $2^{\mathrm{nd}}$ compartment is filled with $1$ mole of ideal diatomic gas at $500 \mathrm{K}$. Initially pressure of gases in both the compartment is same and equal to atmospheric pressure. Temperature of atmosphere is $300 \mathrm{K}$. Finally gases achieve equilibrium. '$R$' is the gas constant

An ideal gas which undergoes through a process $V=a{T}^2;$ starting at $T_0$ and ends at $2T_0$. $a$ is a constant. The molar heat capacity of the gas if it is monoatomic is $\frac{n}{2}R$; What is $n$ ?

The SI unit for heat capacity is joule per kelvin.

Define heat capacity with unit.

For a gas of molecular weight $M$ specific heat capacity at constant pressure is $\left(r=\frac{c_p}{c_v}\right)$

Two litres of water at initial temperature of $27°\mathrm{C}$ is heated by a heater of power $1 \mathrm{kW}$ in a kettle. If the lid of the kettle is open, then heat energy is lost at a constant rate of $160 \mathrm{J} {\mathrm{s}}^{-1}$. The time in which the temperature will rise from $27°\mathrm{C}$ to $77°\mathrm{C}$ is,

(Specific heat of water $=4.2 \mathrm{kJ} {\mathrm{kg}}^{-1} °{\mathrm{C}}^{-1}$)

Why the specific heat at a constant pressure is more than that at constant volume.

What are the two principal specific heats of a gas.

It is the specific heat of a gas at constant pressure, ${\mathrm{C}}_{\mathrm{p}}$ is $\frac{5}{2}\mathrm{R}$The atomicity of the gas would be

What is specific heat of gas at constant pressure

What is Principal Specific Heat of Gas at Constant Volume:

200 g water is heated from ${40}^{\mathrm{ o}}\mathrm{C}$ to ${60}^{\mathrm{ o}}\mathrm{C}$ . Ignoring the slight expansion of water, the change in its internal energy is close to (Given specific heat of water $=4184$ J/kg/K):

A copper ball of mass $100 \mathrm{g}$ is at a temperature $T$. It is dropped in a copper calorimeter of mass $100 \mathrm{g},$ filled with $170 \mathrm{g}$ of water at room temperature. Subsequently, the temperature of the system is found to be ${75}^{\text{o}} \mathrm{C}$. $T$ is given by:
(Given: room temperature = ${30}^{\text{o}}\mathrm{C}$, the specific heat of copper $=0.1\hspace{0.17em}\mathrm{cal} {{\mathrm{g}}^{-1}}^{\mathrm{o}}{\mathrm{C}}^{-1}$)