Specific Heat Capacity

Define specific heat of an object. Write the expressions for heat energy absorbed and lost by an object in terms of specific heat. Explain the process of measurement of specific heat by mixing method in a calorimeter.

Explain measurement of specific heat: Mixing method and calorimeter.

Which principle is used to measure the specific heat capacity of a substance?

The SI unit of specific heat is $\raisebox{1ex}{$\mathrm{J}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{kg} \mathrm{K}$}\right.$.

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

The specific heat capacity of any substance is the amount of heat required to raise the temperature of one unit substance by hundred degree.

The specific heat capacity of water is less than that of steam.

The specific heat capacity of water is less than that of ice.

Name an instrument that works on the principle of heat exchange.

A cube of lead of $500 \mathrm{g}$ at $25 °\mathrm{C}$ is supplied with a $3225 \mathrm{J}$ heat. Find the final temperature (in degree Celsius) of the lead cube. (Take, specific heat of lead is $0.129 \raisebox{1ex}{$\mathrm{J}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{g} °\mathrm{C}$}\right.$) 

Liquid ammonia is used in an ice factory for making ice from water. If the water at $20 ℃$ is to be converted into $2 \mathrm{kg}$ ice at $0 ℃$, how many grams of ammonia is to be evaporated?(Given: The latent heat of vaporization of ammonia $=341 \mathrm{cal}/\mathrm{g}$, The specific latent heat of fusion of water $=80 \raisebox{1ex}{$\mathrm{cal}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{g}$}\right.$, The specific heat capacity of water $=1 \raisebox{1ex}{$\mathrm{cal}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{g} ℃$}\right.$)

Name the instrument used to measure the specific heat capacity of an object.

The specific heat capacity of water is less than that of aluminium.

Calculate the heat energy (in joules) to raise the temperature of $5 \mathrm{kg}$ of water from $20 °\mathrm{C}$ to $100 °\mathrm{C}$. (Take specific heat of water, $s_w=4.2\times {10}^3 \mathrm{J} {\mathrm{kg}}^{-1} {\mathrm{K}}^{-1}$)

A sphere of $0.047 \mathrm{kg}$aluminium is placed for sufficient time in a vessel containing boiling water, so that the sphere is at $100 °\mathrm{C}$. It is then immediately transferred to $0.14 \mathrm{kg}$ copper calorimeter containing $0.25 \mathrm{kg}$ water at $20 °\mathrm{C}$. The temperature of water rises and attains a steady state at $23 °\mathrm{C}$. Calculate the specific heat capacity of aluminium.

A calorimeter has mass $100 \mathrm{g}$ and specific heat $0.1 \mathrm{kcal}/\mathrm{kg}℃$. It contains $250 \mathrm{gm}$ of liquid at $30 ℃$ having a specific heat of $0.4 \mathrm{kcal}/\mathrm{kg}℃$. If we drop a piece of ice of mass $10 \mathrm{g}$ at $0 ℃$, What will be the temperature of the mixture? (Take Specific latent heat of fusion of ice as $80 \raisebox{1ex}{$\mathrm{cal}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{g}$}\right.$)

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

How much heat energy (in $\mathrm{kcal}$) is necessary to raise the temperature of $5 \mathrm{kg}$ of water from $20℃$ to $100℃$?

Specific heat capacity of a substance depends on the mass of the substance. 

Study the table given below and answer the following questions

$78000 \mathrm{J}$ of energy was used to heat up iron by $20°\mathrm{C}$. How much mass of iron was heated?