Home
Class 11
CHEMISTRY
In the reaction equilibrium N(2)O(4) h...

In the reaction equilibrium
`N_(2)O_(4) hArr 2NO_(2)(g)`
When `5` mol of each is taken and the temperature is kept at `298 K`, the total pressure was found to be `20` bar.
Given : `Delta_(f)G_(n_(2)O_(4))^(ɵ)=100 kJ, Delta_(f)G_(NO_(2))^(ɵ)=50 KJ`
a. Find `DeltaG^(ɵ)` of the reaction at `298 K`.
b. Find the direction of the reaction.

Text Solution

Verified by Experts

Reaction quotient `=([p_(NO_(2))]^(2))/([p_(N_(2)O_(4))])=100/10=10`
`DeltaG_("Reaction")^(ɵ)=2Delta_(f)G_(NO_(2))^(ɵ)-Delta_(f)G_(N_(2)O_(4))^(ɵ)`
`=2xx50-100=0`
we know, `DeltaG=DeltaG^(ɵ)-2.303RT log_(10) Q_(p)`
`=0-2.303xx8.314xx298 log 10`
`=-5705.8 J=-5.705 kJ`
Negative value shows that reaction will be in forward direction.
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY ENGLISH|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

In the reaction equilibrium N_(2)O_(4) hArr 2NO_(2)(g) When 5 mol of each is taken and the temperature is kept at 298 K , the total pressure was found to be 20 bar. Given : Delta_(f)G_(n_(2)O_(4))^(ɵ)=100 kJ, Delta_(f)G_(NO_(2))^(ɵ)=50 KJ a. Find DeltaG of the reaction at 298 K . b. Find the direction of the reaction.

In the reaction 2NO(g) hArr N_(2)(g)+O_(2)(g) , the values of K_(c) and K_(p) are ……….. at a given temperature.

For the following equilibrium N_(2)O_(4)(g)hArr 2NO_(2)(g) K_(p) is found to be equal to K_(c) . This is attained when :

In the given reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) , equilibrium means that

For the reaction: N_(2)O_(4)(g) hArr 2NO_(2)(g) (i)" " In a mixture of 5 mol NO_(2) and 5 mol N_(2)O_(4) and pressure of 20 bar. Calculate the value of DeltaG for the reaction. Given DeltaG_(f)^(@) (NO_(2)) = 50 KJ/mol, DeltaG_(f)^(@) ((N_(2)O_(4)) =100 KJ/mol and T=298 K. (ii) Predict the direction in which the reaction will shift, in order to attain equilibrium [Given at T=298 K, 2.303 "RT" = 5.7 KJ/mol.]

For the reaction: N_(2)O_(4)(g) hArr 2NO_(2)(g) (i)" " In a mixture of 5 mol NO_(2) and 5 mol N_(2)O_(4) and pressure of 20 bar. Calculate the value of DeltaG for the reaction. Given DeltaG_(f)^(@) (NO_(2)) = 50 KJ/mol, DeltaG_(f)^(@) ((N_(2)O_(4)) =100 KJ/mol and T=298 K. (ii) Predict the direction in which the reaction will shift, in order to attain equilibrium [Given at T=298 K, 2.303 "RT" = 5.7 KJ/mol.]

The reaction 2NO_(2)(g) hArr N_(2)O_(4)(g) is an exothermic equilibrium . This means that:

For the following gases equilibrium, N_(2)O_(4)(g)hArr2NO_(2)(g) K_(p) is found to be equal to K_(c) . This is attained when:

For the following gases equilibrium, N_(2)O_(4) (g)hArr2NO_(2) (g) , K_(p) is found to be equal to K_(c) . This is attained when:

For the dissociation reaction N_(2)O_(4)(g)hArr2NO_(2)(g), the equilibrium constant K_(P) is 0.120 atm at 298 K and total pressure of system is 2 atm. Calculate the degree of dissociation of N_(2)O_(4) .