Calorimetry

$1 \mathrm{kg}$ water of specific heat $1 \mathrm{cal} {\mathrm{g}}^{-1}{}^{\circ }\mathrm{C}^{-1}$ is kept in a container at $10°\mathrm{C}$. If $500 \mathrm{g}$ of ice at $0°\mathrm{C}$ is required to cool down the water from $10°\mathrm{C}$ to $0°\mathrm{C}$, then what is the water equivalent of the container? (Latent heat of fusion for ice $L=80 \mathrm{cal} {\mathrm{g}}^{-1}$)

Two blocks of ice when pressed together join to
form one block. It happens because

When inflated tyre bursts, the air escaps out.

When salt is properly mixed with ice, the melting point of ice?

A circular disc of copper has a symmetrical hole at its centre. The disc is uniformly heated. The diameter of the hole will

Ice in a freezer is at $-7°\mathrm{C}.100 \mathrm{g}$ of this ice is mixed with $200 \mathrm{g}$ of water at $15°\mathrm{C}$. Take the freezing temperature of water to be $0°\mathrm{C}$, the specific heat of ice equal to $2.2 \mathrm{J}/\mathrm{g}°\mathrm{C},$ specific heat of water equal to$4.2 \mathrm{J}/\mathrm{g}°\mathrm{C}$ and the latent heat of ice equal to $335 \mathrm{J}/\mathrm{g}$.
Assuming no loss of heat to the environment, the mass of ice in the final mixture is closest to
 

Initially, a beaker has $100 \mathrm{g}$ of water at temperature $90 °\mathrm{C}$. Later another $600 \mathrm{g}$ of water at temperature $20 °\mathrm{C}$ was poured into the beaker. The temperature, $T$ of the water after mixing is

If $x \mathrm{gm}$ of steam at $100°\mathrm{C}$ becomes water at $100°\mathrm{C}$ which converts $y \mathrm{gm}$ of ice at $0°\mathrm{C}$ into water at $100°\mathrm{C}$, then the ratio $\frac{x}{y}$ will be,

What is the thermal capacity of a copper calorimeter of mass $40 \mathrm{g}$ and with specific heat $4.2 \mathrm{x} {10}^2 \mathrm{J} {\mathrm{kg}}^{-1} °{\mathrm{C}}^{-1}$?

Find the temperature of the mixture of $1 \mathrm{kg}$ of ice at $0^o$$\mathrm{C}$ and $1 \mathrm{kg}$ of water at ${10}^o$$\mathrm{C}$.

What is the final temperature of the mixture of $540 \mathrm{g}$ of ice at $0^o$$\mathrm{C}$ and $540 \mathrm{g}$ of water at ${80}^o$$\mathrm{C}$.

Under which of the following condition is the following statement defined?

"Calorie is defined as the amount of heat required to raise the temperature of  $1\mathit{ }\mathrm{gm}$ of water by $1^o\mathrm{C}$" 

The whole mixture in the calorimeter become ice if:

Water of volume $2 \mathrm{L}$ in a container is heated with a coil of power $1 \mathrm{kW}$ at $27{ }^0\mathrm{C}$. The lid of the container is open and energy dissipates at rate of $160 \mathrm{J}/\mathrm{s}$. In how much time temperature will rise from $27{ }^0\mathrm{C}$ to $77{ }^0\mathrm{C}$ ? [Given specific heat of water is $4.2 \mathrm{kJ}/\mathrm{kg}$]

$80 \mathrm{gm}$ of water at ${30}^o\mathrm{C}$ is poured on a large block of ice at $0^{\mathrm{o}}\mathrm{C}$. The mass of ice that melts is:

A calorimeter contains $70.2\mathrm{ }\mathrm{g}$ of water at $15.3 °\mathrm{C}$. If $143.7\mathrm{ }\mathrm{g}$ of water at $\text{36.5} °\mathrm{C}$ is mixed with it, the common temperature becomes $28.7 °\mathrm{C}$. The water equivalent of the calorimeter is

$80\mathrm{ }\mathrm{g}$ of water at $30 °\mathrm{C}$ is poured on a large block of ice at $0 °\mathrm{C}$. The mass of ice that melts is

$300 \mathrm{g}$ of water at $25 °\mathrm{C}$ is added to $100 \mathrm{g}$ of ice at $0 °\mathrm{C}$. The final temperature of mixture is

A lead ball at ${30}^{\text{o}}\text{C}$ is dropped from a height of 6.2 km. The ball is heated due to the air resistance and it completely melts just before reaching the ground. The molten substance falls slowly on the ground. If the specific heat of lead $=126\text{k}\text{j}{\text{g}}^{-1}{}^{\text{o}}{\text{C}}^{-1}$ and melting point of lead $={330}^{\text{o}}\text{C}$ and suppose that any mechanical energy lost is used to heat the ball, then the latent heat of fusion of lead is

$\mathrm{A}$ thermos flask contains $250 \mathrm{g}$ of coffee at $90°\mathrm{C}$. To this $20 \mathrm{g}$ of milk at $5°\mathrm{C}$ is added. After equilibrium is established, the temperature of the liquid is (Assume no heat loss to the thermos bottle. Take specific heat of coffee and milk as $\left.1.00\mathrm{cal}/\mathrm{g}°\mathrm{C}\right)$