Home
Class 11
CHEMISTRY
10mol of an ideal gas confined to a volu...

`10mol` of an ideal gas confined to a volume of `10L` is released into atmosphere at `300K` where the pressure is 1bar. The work done by the gas is `(R = 0.083 L "bar" K^(-1)mol^(-1))`

A

`249 L`bar

B

`259 L` bar

C

`239 L`bar

D

`220L` bar

Text Solution

Verified by Experts

Initial volume, `V_(1) = 10L`
`V_(2)("final") = (nRT)/(P) = (10 xx 0.083 xx 300)/(1) = 249 L`
`W = P DeltaV =1 xx (249-10) = 239 L` bar
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Ex 6.3|27 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Ex 6.4|16 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Ex 6.1|26 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

An ideal gas is allowed to expand from 1 L to 10 L against a constant external pressure of 1 bar. Calculate the work done inkJ.

2 mol of chlorine gas occupies a volume of 800 mL at 300 K and 5xx10^(6) Pa pressure. Calculate the compressibility factor of the gas. (R=0.083 L "bar" K^(-1)mol^(-1)) . Comment, whether the gas is more compressible or less compressible under these conditions.

Knowledge Check

  • 10 moles of an ideal gas confined to a volume of 10 L is released into atmosphere at 300 K where the pressure is 1 bar. The work done by the gas is: ltBrgt (R=0.083L" bar "K^(-1)mol^(-1))

    A
    249 L bar
    B
    259 L bar
    C
    239 L bar
    D
    220 L bar

  • 10 mole of an ideal gas at 30^(@) C confined to a volume of 10 L is released into 1 bar. The work done by the gas is:

    A
    249 L bar
    B
    259 L bar
    C
    239 L bar
    D
    220 L bar

  • An ideal gas is allowed to expand from 1L to 10 L against a constant external pressure of 1 bar. The work doen in kJ is:

    A
    `-9.0`
    B
    `+10.0`
    C
    `-0.9`
    D
    `-2.0`

    • Similar Questions

    Explore conceptually related problems

    20 mol of chlorine gas occupies a volume of 800 ml at 300 K and 5 xx 10^(6) Pa pressure. Calculate the compressibility factor of the gas (R = 0.083 L bar K^(-1) mol^(-1) ). Comment whether the gas is more compressible or less compressible under the conditions

    Three grams of non - volatile solute whenn dissolved in a litre of water shows an osmotic pressure of 2 bar at 300K. Calculate the molar mass of the solute . (R = 0.083 L bar K^(-1) mol^(-1) ) .

    4.0 mol of an idela gas initially at 1.5atm and 300K is heated to 600K where the pressure is 4.5atm . Also, C_(vm) = a+bT, a = 25 J K^(-1)mol^(-1), b = 0.03 J K^(-2) mol^(-1) . Determine DeltaU, DeltaH .

    If two moles of an ideal gas at 500 K occupies a volume of 41 litres, the pressure of the gas is (R = 0.082 L atm K^(-1) mol^(-1))

    Under isothermal condition, a gas at 300 K expands from 0.1 L to 0.25 L against a constant external pressure of 2 bar. The work done by the gas is ( Given that 1 L bar= 100J)

    Home
    Profile