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Worksheet: Calorimetry | Physics Class 10 ICSE PDF Download

Part A — Multiple Choice Questions

Q1. The SI unit of heat (energy) is:

(a) Calorie

(b) Joule

(c) Erg

(d) Watt

Q2. When pure ice at 0°C melts to water at 0°C, the temperature of the mixture:

(a) Rises

(b) Falls

(c) Stays constant

(d) Becomes 100°C

Q3. The specific heat capacity of a substance tells us:

(a) Heat needed to raise the body’s temperature by 1°C

(b) Heat needed to raise 1 kilogram of the substance by 1°C

(c) Heat needed to melt 1 kilogram of the substance

(d) Heat released when water freezes

Q4. Coastal places have a moderate climate mainly because water has:

(a) Low specific heat capacity

(b) High specific heat capacity

(c) No specific heat capacity

(d) High latent heat of vaporisation only

Q5. Which statement about impurities is correct?

(a) Impurities increase the melting point

(b) Impurities decrease the melting point

(c) Impurities do not affect the melting point

(d) Impurities make the temperature jump to 100°C

Part B — Short Answer Questions 

Q6. What is heat capacity? How is it different from specific heat capacity?

Q7. Why is a calorimeter made of copper?

Q8. Why do farmers flood fields during a cold night in winter?

Q9. Explain the principle of calorimetry (principle of mixtures).

Q10. What is latent heat? Give one example.

Part C — Long Answer Questions

Q11. How much heat is required to raise the temperature of 200 grams of water from 25°C to 55°C? (Specific heat capacity of water = 4200 J per kg per °C)

Q12. Explain how impurities and pressure affect the melting and boiling points of substances. Give examples.

Q13:How much heat is required to melt 500 g of ice at 0°C into water at 0°C? (Specific latent heat of fusion of ice = 3.34 × 10⁵ J per kg)

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FAQs on Worksheet: Calorimetry - Physics Class 10 ICSE

1. What is calorimetry and how is it used in experiments?
Ans. Calorimetry is the science of measuring the heat transfer associated with chemical reactions or physical changes. It is used in experiments to determine the energy changes that occur during these processes, allowing scientists to calculate the heat absorbed or released. By using a calorimeter, researchers can obtain precise measurements of temperature changes that help in understanding the enthalpy changes of reactions.
2. What are the different types of calorimeters?
Ans. There are several types of calorimeters used in experiments, including: 1. <b>Coffee Cup Calorimeter</b>: A simple and inexpensive device that is often used in classrooms to measure the heat of reaction at constant pressure. 2. <b>Bomb Calorimeter</b>: A more complex apparatus used for measuring the heat of combustion at constant volume, suitable for high-energy reactions. 3. <b>Differential Scanning Calorimeter (DSC)</b>: This instrument measures the heat flow associated with phase transitions in materials as a function of temperature, providing detailed thermal analysis.
3. What is the principle of conservation of energy as it relates to calorimetry?
Ans. The principle of conservation of energy states that energy cannot be created or destroyed, only transformed from one form to another. In calorimetry, this principle is applied by measuring the heat exchanged between a system (e.g., a chemical reaction) and its surroundings. The heat lost by the system is equal to the heat gained by the surroundings, allowing scientists to calculate the total energy change during a reaction.
4. How do you calculate the heat change in a calorimetry experiment?
Ans. The heat change (q) in a calorimetry experiment can be calculated using the formula: q = m × c × ΔT, where m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT is the change in temperature (final temperature - initial temperature). This calculation helps in determining how much energy is absorbed or released during a reaction.
5. Why is it important to know the specific heat capacity of substances in calorimetry?
Ans. Knowing the specific heat capacity of substances is crucial in calorimetry because it allows for accurate calculations of heat transfer. The specific heat capacity is the amount of heat required to raise the temperature of 1 gram of a substance by 1°C. Different substances have different specific heat capacities, which influences how they absorb or release heat during reactions. Accurate knowledge of these values ensures reliable experimental results and interpretations in calorimetry studies.
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