Home
Class 12
CHEMISTRY
The standard Gibbs free energy change (D...

The standard Gibbs free energy change `(DeltaG^(0))` at `25^(@)C` for the dissociation of `N_(2)O_(4)(g)` to `NO_(2)(g)` is (given, equilibrium constant = 0.15, R = 8.314 JK/mol)

A

1.1 kJ

B

4.7 kJ

C

8.1 kJ

D

38.2 kJ

Text Solution

Verified by Experts

Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • QUESTION PAPER 2013

    WB JEE PREVIOUS YEAR PAPER|Exercise CATEGORY-III|5 Videos

  • QUESTION PAPER 2013

    WB JEE PREVIOUS YEAR PAPER|Exercise CATEGORY-III|5 Videos

  • QUESTION PAPER 2012

    WB JEE PREVIOUS YEAR PAPER|Exercise Subject: Chemistry|41 Videos

  • QUESTION PAPER 2015

    WB JEE PREVIOUS YEAR PAPER|Exercise CHEMISTRY (CATEGORY III)|5 Videos

Similar Questions

Explore conceptually related problems

The standard Gibbs free energy (/_\G^(@)) at 25^(@) C for the dissociations of N_2O_4 (g) to NO_2 (g) is (given : equilibrium constant =0.15,R=8.314J*K^(-1)mol^(-1)

Calculate the standard free energy change (DeltaG^@) of the following reaction and say whether it is feasible at 373 K or not 1/2H_(2(g)) + 1/2I_(2(g)) to HI_((g)) , DeltaH_r^@ is + 25.95 kJ "mole"^(-1) . Standard entropies of HI_((g)).H_(2(g)) and I_(2(g)) are 206.3, 130.6 and 116.7 JK^(-1) "mole"^(-1) .

Knowledge Check

  • If the equilibrium constant for N_2(g) + O_2(g) iff 2NO(g) is K, the equilibrium constant for 1/2N_2(g) +1/2 O_2(g) iff NO(g) will be:

    A
    `K^(1/2)`
    B
    1/2K
    C
    K
    D
    `K^2`

  • The reaction, C(s)+H_2O(g)hArrCO(g)+H_2(g) , /_\H>0 , is in equilibrium. At equilibrium-

    A
    if temperature is increased, the partial pressure of `H_2O(g)` will decrease
    B
    concentration of `H_2(g)` will decrease if an inert gas is added at constant temperature and volume
    C
    concentration of CO(g) will increase if pressure is increased at constant temperature
    D
    the equilibrium will move towards right if an inert gas is added at constant temperature and pressure

  • The standard Gibbs energy change at 300 K for the reaction 2A iff B+C is 2494.2 J. At a given time, the composition of the reaction mixture is [A] =1/2, [B] = 2 and [C] = 1/2. The reaction proceeds in the:[R = 8.314 JK/mol,e = 2.718]

    A
    reverse direction because `Q gt K_c`
    B
    forward direction because `Q lt K_c`
    C
    reverse direction because `Q lt K_c`
    D
    forward direction because `Q gt K_c`

    • Similar Questions

    Explore conceptually related problems

    At 200^(@)C , the equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) is achieved in the following two pathways: (i) 0.1 mol N_(2)O_(4) is heated in a closed vassel of 1 L volume. (ii) a mixture of 0.05 mol N_(2)O_(4) (g) and 0.05 mol NO_(2)(g) is heated at 200^(@)C in a closed vessel of 1 L volume. in these two cases, will the equilibrium concentrations of N_(2)O_(4)(g) and NO_(2)(g) and the values of equilibrium constants be the same?

    Equilibrium constant for a reaction 1.6xx10^(-6) at 298K. Calculate standard free energy change (DeltaG^(0)) and standard entropy change (DeltaS^(0)) of the reaction wat that pressure. Given, at 298K, DeltaH^(0)=25.34kJ .

    In the given reaction, calculate standard free energy change at 25^(@)C:2NO(g)+O_(2)(g)to 2NO_(2)(g) . Is the reaction spontaneous under standard conditios? [Given: At 25^(@)C,DeltaG_(f)^(0)[NO(g)]=88.57kJ*mol^(-1) and DeltaG_(f)^(0)[NO_(2)(g)]=51.30kJ*mol^(-1) .

    Calculate the DeltaG^0 for the reaction N_2(g) + O_2(g) * 2NO(g) Given DeltaH^0 =180.5 K.J , and DeltaS^0 = 15 J at 25^@C .

    The standard Gibbs energy change at 300K for the reaction 2A⇋B+C is 2494.2 J. At a given time, the composition of the reaction mixture is [A] = 2 1 ​ , [B] = 2 and [C] = 2 1 ​ . The reaction proceeds in the : [R=8.314J/K/mol,e=2.718]

    Home
    Profile