Question
2 moles of an ideal gas is expanded isothermally and reversibly from 1 litre of 10 litre at 300 K . The enthalpy change (in kJ ) for the process is(a) 11.4 kJ(b) -11.4 kJ(c) 0 kJ(d) 4.8 kJ .
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The problem states that the gas is expanded isothermally and reversibly. In an isothermal process, the temperature remains constant. Show more…
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Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litres at $300 \mathrm{~K}$. The enthalpy change (in $\mathrm{kJ}$ ) for the process is [2004S] (a) $11.4 \mathrm{~kJ}$ (b) $-11.4 \mathrm{~kJ}$ (c) $0 \mathrm{~kJ}$ (d) $4.8 \mathrm{~kJ}$
Thermodynamics
Topic 1 : Thermodynamics
Two mole of an ideal gas is expanded isothermally and reversibly from 1 litre of 10 litre at $300 \mathrm{~K}$. The enthalpy change (in $\mathrm{kJ}$ ) for the process is a. $11.4 \mathrm{~kJ}$ b. $-11.4 \mathrm{~kJ}$ c. $0 \mathrm{~kJ}$ d. $4.8 \mathrm{~kJ}$. [IIT 2004]
Two moles of an ideal gas undergo expansion in volume at 37°C from 2 L to 20 L isothermally and reversibly. The enthalpy change in the process is -11.87 kJ + 11.87 kJ + 0 kJ - 6.25 kJ.
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