Class 10 Calorimetry Mock Test (ICSE)

Topics in Calorimetry

• Heat capacity and specific heat capacity
• Principle of method of mixtures
• Latent heat of fusion and vaporisation
• Heating curve of ice
• Natural consequences of high specific heat of water

Calorimetry practice questions with answers

1. Q1Multiple choice·1 mark
   The SI unit of specific heat capacity is:

   1. (a)$\text{J kg}^{-1}\text{ K}$
   2. (b)$\text{J kg}^{-2}\text{ K}^{-1}$
   3. (c)$\text{J kg K}^{-1}$
   4. (d)$\text{J kg}^{-1}\text{ K}^{-1}$
   Show answer and step marks

   1. Correct option: (d)+1

   Answer: (d)
2. Q2Multiple choice·1 mark
   During the process of heating ice from $-10^\circ\text{C}$ to steam at $100^\circ\text{C}$, the temperature remains constant at:

   1. (a)All temperatures between $0^\circ\text{C}$ and $100^\circ\text{C}$
   2. (b)$-10^\circ\text{C}$ only
   3. (c)$0^\circ\text{C}$ and $100^\circ\text{C}$
   4. (d)$0^\circ\text{C}$ only
   Show answer and step marks

   1. Correct option: (c)+1

   Answer: (c)
3. Q3Multiple choice·1 mark
   Water is commonly used as an effective coolant in automobile radiators because:

   1. (a)It is cheap and easily available.
   2. (b)It has a high specific latent heat of vaporization.
   3. (c)It has a high specific heat capacity, allowing it to absorb large amounts of heat with a small rise in temperature.
   4. (d)It has a very low thermal conductivity.
   Show answer and step marks

   1. Correct option: (c)+1

   Answer: (c)
4. Q4Multiple choice·1 mark
   The specific latent heat of fusion of ice is $3.36 \times 10^5\text{ J kg}^{-1}$. What does this statement signify?

   1. (a)$1\text{ kg}$ of water at $100^\circ\text{C}$ absorbs $3.36 \times 10^5\text{ J}$ of heat to completely convert into steam at $100^\circ\text{C}$.
   2. (b)$1\text{ kg}$ of ice requires $3.36 \times 10^5\text{ J}$ of heat to raise its temperature by $1^\circ\text{C}$.
   3. (c)$1\text{ kg}$ of ice at $0^\circ\text{C}$ absorbs $3.36 \times 10^5\text{ J}$ of heat to completely convert into water at $0^\circ\text{C}$.
   4. (d)$1\text{ g}$ of ice at $0^\circ\text{C}$ absorbs $3.36 \times 10^5\text{ J}$ of heat to melt into water.
   Show answer and step marks

   1. Correct option: (c) $1\text{ kg}$ of ice at $0^\circ\text{C}$ absorbs $3.36 \times 10^5\text{ J}$ of heat to completely convert into water at $0^\circ\text{C}$.+1

   Answer: (c)
5. Q5Long answer·4 marks
   (a) State the meaning of the statement: "Specific latent heat of vaporisation of water is $2268\text{ J g}^{-1}$." (b) Calculate the total heat energy required to melt $50\text{ g}$ of ice at $0\text{ }^\circ\text{C}$ and raise the temperature of the resulting water to $80\text{ }^\circ\text{C}$. (Given: Specific latent heat of ice $= 336\text{ J g}^{-1}$, Specific heat capacity of water $= 4.2\text{ J g}^{-1}\text{ }^\circ\text{C}^{-1}$)
   Show answer and step marks

   1. (a) It means that $2268\text{ J}$ of heat energy is required to convert $1\text{ g}$ of water at $100\text{ }^\circ\text{C}$ into steam at $100\text{ }^\circ\text{C}$ without any change in temperature.+1
   2. (b) Heat required to melt ice at $0\text{ }^\circ\text{C}$ to water at $0\text{ }^\circ\text{C}$: $Q_1 = m \cdot L = 50\text{ g} \times 336\text{ J g}^{-1} = 16800\text{ J}$.+1
   3. Heat required to raise the temperature of water from $0\text{ }^\circ\text{C}$ to $80\text{ }^\circ\text{C}$: $Q_2 = m \cdot c \cdot \Delta t = 50\text{ g} \times 4.2\text{ J g}^{-1}\text{ }^\circ\text{C}^{-1} \times 80\text{ }^\circ\text{C} = 16800\text{ J}$.+1
   4. Total heat energy required: $Q = Q_1 + Q_2 = 16800\text{ J} + 16800\text{ J} = 33600\text{ J}$ (or $33.6\text{ kJ}$).+1

   Answer: (a) $2268\text{ J}$ of heat is needed to change $1\text{ g}$ of water at $100\text{ }^\circ\text{C}$ into steam at $100\text{ }^\circ\text{C}$ without any change in temperature. (b) $33600\text{ J}$ (or $33.6\text{ kJ}$)

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