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The maximum work done when pressure of ...

The maximum work done when pressure of n moles of `H_(2)` was reduced from 20 atm to 1 atm at constant temperature of 273 K is found to be 8180 calories. What is the value of n?

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Calculate the maximum work done when pressure on 10 g of hydrogen is reduces from 20 atm to 1 atm at a constant temperature of 273 K . The gas behaves ideally. Will there be any change in internal energy? Also, calculate 'q' .

Calculate the maximum work done when pressure on 10 g of hydrogen is reduced from 20 to 1 atm at a constant temperature of 273 K. The gas behaves ideally. Will there be any change in internal energy ? Also, calculate 'q'.

Knowledge Check

  • The maximum work done when pressure on 10 g of hydrogen is reduced from 20 to 1 atm at a constant temeprature of 273 will be

    A
    8170 cal
    B
    8180 cal
    C
    8200 cal
    D
    8350 cal

  • What will be the value of maximum work one by the gas when pressure of 20 gm H_(2) is reduced from 20 to 2 atm at constant tempreature of 300 k, assuming gas to behave ideally?

    A
    57.44 kJ
    B
    114.88 J
    C
    224.478 kJ
    D
    22.4478 kJ

  • In a vessel, the pressure of a gas varies directly with its temperature, if its volume is kept constant, when the pressure is increased from 1 atm to 3 atm, then the temperature increases from 273 K to 'x' K. What is the value of x, if volume ix kept constant?

    A
    91K
    B
    546 K
    C
    819 K
    D
    900 K

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    Calculate the maximum work down when pressure on 10g of hydrogen is reduced from 20 to 1atm at a constant temperature of 273K . The gas behaves ideally. Will there be any change in internal energy. Also calculate q. (R = 2 cal K^(-1) mol^(-1))

    In a vessel, the pressure of a gas varies directly with its temperature, if its volume is kept constant. When the pressure is increased from 1 atm to 3 atm, then the temperature increases from 273 K to 'x' K. What is the value of x, if volume is kept constant?

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