Heat Capacity, Specific Heat Capacity and Its Measurement

The total heat needed to heat $1 \mathrm{kg}$ of ice at $-10º\mathrm{C}$ to water at $100º\mathrm{C}$ is $7.77 \times {10}^5 \mathrm{J}$. Calculate the specific latent heat of ice.

Specific heat capacity of ice $=2100 \mathrm{J} {\mathrm{kg}}^{-1}{\mathrm{K}}^{-1}$

Specific heat capacity of water $=4200 \mathrm{J} {\mathrm{kg}}^{-1}{\mathrm{K}}^{-1}$

Calculate the total amount of heat energy required to convert $100 \mathrm{g}$ of ice at $-10℃$ completely into water at $100℃$. Specific heat capacity of ice $=2.1 \mathrm{J} {\mathrm{g}}^{-1}{\mathrm{K}}^{-1}$, specific heat capacity of water is $4.2 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$ , specific latent heat of ice is $=336 \mathrm{J} {\mathrm{g}}^{-1}$

$2 \mathrm{kg}$ of ice melts when water at $100℃$ is poured in a hole drilled in a block of ice. What is the mass of water that was used? Given: Specific heat capacity of water $4200 \mathrm{J} {\mathrm{kg}}^{-1}{\mathrm{K}}^{-1}$, $L_{ice}=336\times {10}^3 \mathrm{J} {\mathrm{kg}}^{-1}.$

$250 \mathrm{g}$ of water at $30° \mathrm{C}$ is present in a copper vessel of mass $50 \mathrm{g}$. Calculate the mass of ice required to bring down the temperature of the vessel and its contents to $5° \mathrm{C}$.(Take, specific latent heat of fusion of ice = $336\times {10}^3 \mathrm{J} {\mathrm{kg}}^{-1}$, specific heat capacity of copper vessel = $400 \mathrm{J} {\mathrm{kg}}^{-1} °{\mathrm{C}}^{-1}$ and specific heat capacity of water = $4200 \mathrm{J} {\mathrm{kg}}^{-1} °{\mathrm{C}}^{-1}$).

Find the result of mixing $10 \mathrm{g}$ of ice at $- 10℃$ with $10 \mathrm{g}$ of water at $10℃$. Specific heat capacity of ice $=2.1 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$, Specific latent heat of ice is $=336 \mathrm{J} {\mathrm{g}}^{-1}$ and specific heat capacity of water is $=4.2 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$.

In an experiment, $17 \mathrm{g}$ of ice is used to bring down the temperature of $40 \mathrm{g}$ of water at $34℃$ to its freezing temperature. The specific heat capacity of water is `$4.2 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$. Calculate the specific latent heat of ice. State one important assumption made in the above calculation.

A refrigerator converts $100 \mathrm{g}$ of water at $20℃$ to ice at $–10℃$ in $73.5 \mathrm{minutes}$. Calculate the average rate of heat extraction in $\mathrm{watt}.$ The specific heat capacity of water is $4.2 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$, Specific latent heat of ice is $336 \mathrm{J} {\mathrm{g}}^{-1}$ and the specific heat capacity of ice is $2.1 \mathrm{J} {\mathrm{g}}^{-1}{\mathrm{K}}^{-1}.$

A molten metal of mass $150 \mathrm{g}$ is kept at its melting point $800℃.$ When it is allowed to freeze at the same temperature, it gives out $75,000 \mathrm{J}$ of heat energy.
What is the specific latent heat of the metal?

How much heat energy is released when $5.0 \mathrm{g}$ of water at $20℃$ changes into ice at $0℃$? Take specific heat capacity of water as $4.2 \mathrm{J} {\mathrm{g}}^{-1}{\mathrm{K}}^{-1}$ and  Specific latent heat of fusion of ice $336 \mathrm{J} {\mathrm{g}}^{-1}$.

$10 \mathrm{g}$ of ice at $0 °\mathrm{C}$ absorbs $5460 \mathrm{J}$ of heat energy to melt and change to water at $50℃.$Calculate the specific latent heat of fusion of ice. Specific heat capacity of water is $4200 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$.

The heat supplied to a substance during its change of state, does not cause any rise in its temperature. Why?

The surrounding become pleasantly warm when water in a lake starts freezing in cold countries. Why?

The temperature of the surrounding starts falling when ice in a frozen lake starts melting. Give reason.

It is generally cold after a hail-storm then during and before the hail storm. Give reason.

Ice cream appears cooler to the mouth than water at $0 ℃$. Give reason.

Which requires more heat: $1 \mathrm{g}$ ice at $0 ℃$or $1 \mathrm{g}$ water at $0 ℃$ to raise its temperature to $10 ℃$? Explain.

Which has more heat: $1 \mathrm{g}$ice at $0 °\mathrm{C}$ or $1 \mathrm{g}$ water at $0 °\mathrm{C}$? Give reason.

$1 \mathrm{g}$ ice of $0℃$ melts to form $1 \mathrm{g}$ water at $0℃$. State whether the latent heat is absorbed or given out by ice.

The specific latent heat of fusion of ice is $336 \mathrm{J} {\mathrm{g}}^{-\mathrm{1. }}$Explain the meaning of its statement.

Write the approximate value of specific latent heat of ice.