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The amount of heat required to raise the temperature of 1 kg of water through 1oC is called
- a)specific heat at constant volume
- b)specific heat at constant pressure
- c)kilocalorie
- d)None of these
Correct answer is option 'C'. Can you explain this answer?
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The amount of heat required to raise the temperature of 1 kg of water...
The small calorie or gram calorie (symbol: cal) is the approximate amount of energy needed to raise the temperature of one gram of water by one degree Celsius, thus 1 kilo calorie is the amount of heat required to raise the temperature of 1 kg of water through 1oC
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The amount of heat required to raise the temperature of 1 kg of water...
Understanding Specific Heat
The concept of specific heat is crucial in thermodynamics, particularly when it comes to understanding how substances absorb or release heat.
What is Specific Heat?
- Specific heat is defined as the amount of heat required to raise the temperature of a unit mass of a substance by 1 degree Celsius.
- It is typically expressed in units of joules per kilogram per degree Celsius (J/kg°C) or calories per gram per degree Celsius.
Heat Required for Water
- For water, the specific heat is notably high, which means it requires a substantial amount of energy to change its temperature.
- The specific heat of water is approximately 4.18 J/g°C or 1 cal/g°C, indicating that it takes 1 kilocalorie (kcal) to raise the temperature of 1 kg of water by 1°C.
Correct Option: Kilocalorie
- The correct answer to the question is option 'C', kilocalorie.
- This unit is often used in food and nutrition, representing the energy needed to raise the temperature of 1 kg of water by 1°C.
Why Not Other Options?
- a) Specific heat at constant volume: This refers to a different condition where the volume of the substance does not change, which is not applicable for water in this context.
- b) Specific heat at constant pressure: This is relevant in thermodynamic processes but still does not directly answer the question regarding the heat needed for a temperature change in water.
- d) None of these: This option is incorrect since kilocalorie is indeed the proper term.
In summary, raising the temperature of 1 kg of water by 1°C requires 1 kilocalorie, making option 'C' the correct answer.
The concept of specific heat is crucial in thermodynamics, particularly when it comes to understanding how substances absorb or release heat.
What is Specific Heat?
- Specific heat is defined as the amount of heat required to raise the temperature of a unit mass of a substance by 1 degree Celsius.
- It is typically expressed in units of joules per kilogram per degree Celsius (J/kg°C) or calories per gram per degree Celsius.
Heat Required for Water
- For water, the specific heat is notably high, which means it requires a substantial amount of energy to change its temperature.
- The specific heat of water is approximately 4.18 J/g°C or 1 cal/g°C, indicating that it takes 1 kilocalorie (kcal) to raise the temperature of 1 kg of water by 1°C.
Correct Option: Kilocalorie
- The correct answer to the question is option 'C', kilocalorie.
- This unit is often used in food and nutrition, representing the energy needed to raise the temperature of 1 kg of water by 1°C.
Why Not Other Options?
- a) Specific heat at constant volume: This refers to a different condition where the volume of the substance does not change, which is not applicable for water in this context.
- b) Specific heat at constant pressure: This is relevant in thermodynamic processes but still does not directly answer the question regarding the heat needed for a temperature change in water.
- d) None of these: This option is incorrect since kilocalorie is indeed the proper term.
In summary, raising the temperature of 1 kg of water by 1°C requires 1 kilocalorie, making option 'C' the correct answer.
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The amount of heat required to raise the temperature of 1 kg of water through 1oC is calleda)specific heat at constant volumeb)specific heat at constant pressurec)kilocaloried)None of theseCorrect answer is option 'C'. Can you explain this answer?
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