Home
Class 12
CHEMISTRY
A sample of 3.0 mole of perfect gas at 2...

A sample of `3.0` mole of perfect gas at `200 K` and `2.0 atm` is compressed reversibly and adiabatically until the temperature reaches `250 K`. Given that molar heat capacity at `27.5 J K^(-1) mol^(-1)` at constant volume calculate `q,W,DeltaU,DeltaH` and the final pressure and volume.

Text Solution

AI Generated Solution

To solve the problem step by step, we will calculate the required values: \( q \), \( W \), \( \Delta U \), \( \Delta H \), and the final pressure and volume of the gas. ### Given Data: - Number of moles, \( n = 3.0 \) moles - Initial temperature, \( T_1 = 200 \, K \) - Final temperature, \( T_2 = 250 \, K \) - Initial pressure, \( P_1 = 2.0 \, atm \) - Molar heat capacity at constant volume, \( C_V = 27.5 \, J \, K^{-1} \, mol^{-1} \) ...
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    VMC MODULES ENGLISH|Exercise LEVEL-1|75 Videos

  • THERMODYNAMICS

    VMC MODULES ENGLISH|Exercise LEVEL-2|50 Videos

  • THERMODYNAMICS

    VMC MODULES ENGLISH|Exercise LEVEL-0 (SHORT ANSWER TYPE-II (3 MAKRS))|6 Videos

  • THERMOCHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE ADVANCED (ARCHIVE)|31 Videos

  • THERMODYNAMICS & THERMOCHEMISTRY

    VMC MODULES ENGLISH|Exercise Impeccable|48 Videos

Similar Questions

Explore conceptually related problems

1 mole of an ideal gas at 25^(@) C is subjected to expand reversibly and adiabatically to ten times of its initial volume. Calculate the change in entropy during expansion (in J K^(-1) mol^(-1) )

Volume of 1.5 mole of a gas at 1 atm. pressure and 273K is

A gas originally at 1.10atm and 298K underwent a reversible adiabatic expansion to 1.00atm and 287K . What is the molar heat capacity of the gas?

A vessel of volume 0.2 m^(3) contains hydrogen gas at temperature 300 K and pressure 1 bar. Find the heat required to raise the temperature to 400 K. The molar heat capacity of hydrogen at constant volume is 5 cal//mol K .

A sample of organ gas at 1atm pressure and 27^(@)C expands reversibly and adiabatically from 1.25 dm^(3) to 2.50 dm^(3) . Calculate the enthalpy change in this process. C_(vm) for orgon is 12.48J K^(-1) mol^(-1) .

1mol of an ideal gas at 400K and 10atm is allowed to expand, adiabatically, against 2.0atm external pressure. Find the final temperature of the gas. [Use: C_(v) = (5)/(2)R]

5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K. If Delta U is 14 kJ, what is Delta pV in J ? for this process ( R = 8.0J K ^( -1 ) mol^( -1) )

5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K. If C_V = 28 JK^(-1) mol^(-1) , calculate DeltaU and DeltapV .

A closed vessel of volume 0.2m^3 contain hydrogen gas at temperature 300 K and pressure 10^5 Pa . Then the heat required to raise temperature to 600 K is:(molar heat capacity of hydrogen at constant volume is 5 cal//mol-K )

A sample of argon gas at 1atm pressure and 27^(@)C expands reversibly and adiabatically from 1.25 dm^(3) to 2.50 dm^(3) . Calculate the enthalpy change in this process. C_(v,m) for argon is 12.48J K^(-1) mol^(-1) .