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Heat obtained due to expansion of 1 mol of H2 gas at 1000 K from 10 L to 100 L Video Lecture - JEE
FAQs on Heat obtained due to expansion of 1 mol of H2 gas at 1000 K from 10 L to 100 L Video Lecture - JEE
| 1. How do I calculate the heat obtained due to the expansion of a gas? |  |
Ans. The heat obtained due to the expansion of a gas can be calculated using the formula Q = nCpΔT, where Q is the heat obtained, n is the number of moles of the gas, Cp is the molar heat capacity at constant pressure, and ΔT is the change in temperature.
| 2. What is the molar heat capacity at constant pressure? | |
Ans. The molar heat capacity at constant pressure (Cp) is the amount of heat required to raise the temperature of one mole of a substance by one degree Celsius at constant pressure. It is a property that depends on the nature of the substance.
| 3. How do I calculate the change in temperature during the expansion of a gas? | |
Ans. The change in temperature (ΔT) during the expansion of a gas can be calculated using the formula ΔT = Tf - Ti, where Tf is the final temperature and Ti is the initial temperature.
| 4. Can the heat obtained during the expansion of a gas be negative? | |
Ans. Yes, the heat obtained during the expansion of a gas can be negative. A negative value indicates that heat is lost by the system during the expansion process.
| 5. Is the heat obtained during the expansion of a gas the same as the work done by the gas? | |
Ans. No, the heat obtained during the expansion of a gas is not the same as the work done by the gas. Heat is a form of energy transfer, while work is the energy transferred by a force acting through a distance. The heat obtained is related to the change in temperature, while the work done is related to the change in volume.
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Nov 15, 2024 Last updated |
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