Home
Class 11
CHEMISTRY
For the reaction at 300 K A(g)hArrV(g)...

For the reaction at `300 K`
`A(g)hArrV(g)+S(g)`
`Delta_(r)H^(@)=-30kJ//mol, Delta_(r)S^(@)=-0.1kJK^(-1).mol^(-1)`
What is the value of equilibrium constant ?

A

0

B

1

C

10

D

`+RT`

Text Solution

Verified by Experts

The correct Answer is:
2
`Delta_(r)G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@)`
`=-30+300xx0.1=0`
`Delta_(r)G^(@)=-2.303RTlog K`
`K=1`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    RESONANCE ENGLISH|Exercise INORGANIC CHEMISTRY(Metallurgy)|40 Videos

  • CHEMICAL EQUILIBRIUM

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Alkyl Halide, Alcohol,Phenol,Ether)|27 Videos

  • CHEMICAL BONDING

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Fundamental Concept )|6 Videos

  • D & F-BLOCK ELEMENTS & THEIR IMPORTANT COMPOUNDS

    RESONANCE ENGLISH|Exercise Match the column|1 Videos

Similar Questions

Explore conceptually related problems

For the reaction at 298K: A_((g)) +B_((g)) hArr C_((g)) + D_((g)) Delta H^(@) + 29.8kcal and Delta S^(@) = 100cal K^(-1) . Find the value of equilibrium constant.

For the reaction at 300 K , A(g) rarr B(g) + E(g), DeltaH^(@) = -30 KJ mol^(-1) , the decrease in standard entropy is 0.1 KJK^(-1)mol^(-1) .The equilibrium constant K for the reaction is ________.

The reaction, MgO(s) + C(s) to Mg(s) + CO(g), for which Delta_(r)H^(@)= +491.1 " " kJ " " mol^(-1) and Delta_(r)S^(@)= 198.0 JK^(-1)mol^(-1) , is not feasible at 289 K . Temperature above which reaction will be feasible is :

The reaction, MgO(s) + C(s) to Mg(s) + CO(g), for which Delta_(r)H^(@)= +491.1 " " kJ " " mol^(-1) and Delta_(r)S^(@)= 198.0 JK^(-1)mol^(-1) , is not feasible at 289 K . Temperature above which reaction will be feasible is :

DeltaH^(Theta) and DeltaS^(Theta) for the reaction: Br_(2)(l) +CI_(2)(g) hArr 2BrCI(g) at 298K are 29.3 kJ mol^(-1) and 104.1 J K^(-1) mol^(-1) , respectively. Calculate the equilibrium constant for the reaction.

Calculate the value of equilibrium constant, K for the following reaction at 400 K. 2NOCl(g) hArr 2NO (g) + Cl_2(g) DeltaH^@ = 80.0 kJ mol^(-1), DeltaS^@ = 120 KJ^(-1) mol^(-1) at 400 K, R = 8.31 JK^(-1) mol^(-1) .

Delta_(vap)H = 30 kJ mol^(-1) and Delta_(vap)S = 75Jmol^(-1)K^(-1) . Find the temperature of vapour, at 1 atm.

Predict whether it is possible or not to reduce magnesium oxide using carbon at 298K according to the reaction. MgO(s) +C(s) rarr Mg(s) +CO(g) Delta_(r)H^(Theta) = +491.18 kJ mol^(-1) and Delta_(r)S^(Theta) = 197.67 J K^(-1) mol^(-1) If not at what temperature, the reaction becomes spontaneous.

What is the equilibrium constant K_(c) for the following reaction at 400K ? 2NOCI(g) hArr 2NO(g) +CI_(2)(g) DeltaH^(Theta) = 77.2 kJ mol^(-1) and DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K .

For a demerization reaction , 2A (g) to A_2 (g) at 298 K, Delta U(Theta) = - 20 kJ"mol"^(-1), Delta S^(Theta) = - 30 JK^(-1) "mol"^(-1) , then the Delta G^(Theta) will be _________J.