Home
Class 12
CHEMISTRY
For the reaction N(2)(g) + 3H(2) rarr 2N...

For the reaction `N_(2)(g) + 3H_(2) rarr 2NH_(3)(g)`
`Delta H = - 95.4 kJ and Delta S = -198.3 JK^(-1)`
Calculate the temperature at which Gibbs energy change `(Delta G)` is equal to zero. Predict the nature of the reaction at this temperature and above it.

A

362 K

B

312 K

C

481 K

D

1023 K

Text Solution

Verified by Experts

`Delta G = Delta H-T Delta S " When " Delta G = 0`
`Delta H = T Delta S rArr T = (Delta H)/(Delta S)rArr (-95.4xx1000)/(-198.3)=481 K`
Promotional Banner

Similar Questions

Explore conceptually related problems

For the reaction N_(2)(g) + 3 H_(2) rightarrow 2NH_(3)(g) Delta H = -85.4 kJ and Delta S = - 188.3 Jk^(-1) Calculate the temperature at which Gibs energy change( Delta G ) is equal to zero. Predict the nature of the reaction at this temperature and above it.

For the reaction, N_(2)(g) +3H_(2)(g) rarr 2NH_(3)(g) DeltaH =- 95.0 kJ and DeltaS = - 19000 J K^(-1) Calculate the temperature in centigrade at which it will attain equilibrium.

For reaction, N_(2(g))+3H_(2(g))to2NH_(3(g)) , DeltaH=-95.4kJ and DeltaS=-198.3JK^(-1) . Calculate the maximum temperature at which the reaction will proceed in forward direction.

For a hypothetical reaction A(g) + 3B(g) to 2C(g). Delta H = -100 kJ and Delta S = -200 Jk^(-1) . Then the temperature at which the reaction will be in equilibrium is

For the reaction, A(s) + 3B(g) rarr 4C(g) + d(l) Delta H and Delta U are related as :

For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-