Specific Heat Capacity

Two different liquids of same mass are kept in two identical vessel, which are placed in a freezer that extracts heat from them at the same rate causing each liquid to transform into a solid. The schematic figure below shows the temperaure $T$ vs time $t$ plot for the two materials. We denote the specific heat in the liquid states to be $C_{L1}$ and $C_{L2}$ for materials $1$ and $2$ respectively, and latent heats of fusion $U_1$ and $U_2$ respectively.

Choose the correct option.

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):

Water is used as a coolant because 

A person weighing $50 \mathrm{kg}$ takes in $1500 \mathrm{kcal}$ diet per day. If this energy were to be used in heating the body of person without any losses, then the rise in his temperature is (specific heat of human body $=0.83 \mathrm{c}\mathrm{a}\mathrm{l}\mathrm{ }{\mathrm{g}}^{-1} {\mathrm{℃}}^{-1}$ )

Amongst object A and B, if the specific heat of object A is less than of object B, then 

The amount of heat required to raise the temperature of $1 \mathrm{kg}$ mass of water through $1 \mathrm{K}$ is called its

The amount of heat required to raise the temperature of $1 \mathrm{kg}$ mass of water through $1 \mathrm{K}$ is called its

Specific heat of a substance is given by $S=(1+2T) \mathrm{J} {\mathrm{kg}}^{-1} {\mathrm{K}}^{-1}$, find out amount of heat required to raise the temperature of $2 \mathrm{kg}$ substance from $10°\mathrm{C}$ to $20°\mathrm{C}.$

The number of degrees of freedom of a gas whose specific heat capacity at constant pressure is $33.24 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1},$ is
(universal gas constant $=8.31 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$ )

$20 \mathrm{gm}$ ice at $-10°\mathrm{C}$ is mixed with $m \mathrm{gm}$ steam at $100°\mathrm{C}$. The minimum value of $\mathrm{m}$ so that finally all ice and steam converts into water is,

(Use, $s_{\text{ice}}=0.5 \mathrm{cal} {\mathrm{gm}}^{-1} °\mathrm{C}\text{,} s_{\text{water}}=1 \mathrm{cal} {\mathrm{gm}}^{-1} °\mathrm{C}$, $L$(melting)$=80 \mathrm{cal} {\mathrm{gm}}^{-1}$ and $L$ (vaporization)$=540 \mathrm{cal} {\mathrm{gm}}^{-1}$.)

Which statement is false for specific heat of water?

During illness an $80 \mathrm{kg}$ man ran a fever of $102.2 °\mathrm{F}$ instead of normal body temperature of $98.6 °\mathrm{F}.$ Assuming that the human body is mostly water, how much heat is required to raise his temperature by that amount?

A source of heat supplies heat at a constant rate to a solid cube. The slope of portion $\mathrm{CD}$ of the graphs gives :-

Calculate the change of heat when $5 \mathrm{kg}$ of water at ${20}^{°}$$\mathrm{C}$ is heated to $100°\mathrm{C}$? (specific heat of water $-4.2 \mathrm{kJ} {\mathrm{kg}}^{-1 °}{\mathrm{C}}^{-1}$)

In a mixture of two gases, we have $1$ mole of a certain gas having $\gamma =\frac{7}{5}$ and $1$ mole of another gas having $\gamma =\frac{4}{3}$. Calculate the value of $\gamma$ for the given mixture of gases.

It is known that the universal gas constant $R$ is $n$ times $C_p$ (molar heat capacity at constant pressure) for an ideal monatomic gas. What is the value of $n$ here?

 The temperature of $5$ moles of a gas is changed from ${100}^{o}C$ to ${120}^{o}C$ under isochoric process and internal energy is changed by $80 J.$ The $C_v$ of the gas is

What is the significance of infinite heat capacity of a substance?

Water is used as a coolant because