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Calculate the work done when `1.0` mol of water at `373K` vaporises against an atmosheric pressure of `1.0atm`. Assume ideal gas behaviour.

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Volume of water vapour `=(nRT)/(P) = (1xx0.082 xx 373)/(1.0)`
`= 30.592L`
`DeltaV = 30.59 - 0 = 30.59L`
`w = 1atm xx 30.59L =- 30.59Latm`
`w =- 30.59 xx 101.3J =- 3100J =- 3.1kJ`
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CENGAGE CHEMISTRY ENGLISH-THERMODYNAMICS-Ex 6.1
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  2. During a process, the internal energy of the system increases by 240kJ...

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  3. Calculate the work done when 1.0 mol of water at 373K vaporises agains...

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  4. What will be the volume change if 607.8 J of work is done by a system ...

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  5. 500cm^(3) of a sample of an ideal gas is compressed by an average pres...

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  6. Three moles of an ideal gas are expanded isothermally and reversibly a...

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  7. 2.8g of N(2) gas at 300K and 20atm was allowed to expand isothermally ...

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  8. State whther each of the following will increase or decreases the tota...

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  9. Two moles of an idela gas at 2atm and 27^(@)C is compressed isothermal...

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  10. A simple of gas present in a cylinder fitted with a frictionless pisto...

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  11. One mole of an ideal mono-atomic gas at 27^(@)C expands adiabatically ...

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  13. Adiabatic expansion of an ideal gas is accompanied by

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  14. For a cyclic process, which of the following is true?

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  15. One mole of a gas is heated at constant pressure to raise its temperat...

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  16. What work is to be done on 2mol of a perfect gas at 27^(@)C it is comp...

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  17. 1mol of an ideal gas undergoes reversible isothermal expansion form an...

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  18. A sample of 2kg of helium (assumed ideal) is taken through the process...

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  19. An ideal diatomic gas is caused to pass throguh a cycle shown on the P...

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