Home
Class 11
CHEMISTRY
Equilibrium constant, K(c) for the react...

Equilibrium constant, `K_(c)` for the reaction,
`N_(2(g))+3H_(2(g))hArr2NH_(3(g))`,
at `500 K` is `0.061 litre^(2) "mole"^(-2)`. At a particular time, the analysis shows that composition of the reaction mixture is `3.00 mol litre^(-1)N_(2)`, `2.00 mol litre^(-1)H_(2)`, and `0.500 mol litre^(-1)NH_(3)`. Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?

Promotional Banner

Similar Questions

Explore conceptually related problems

Equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) at 500K is 0.061 At particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^(-1)N_(2) , 2.0 mol L^(-1)H_(2) and 0.5 mol L^(-1)NH_(3) . Is the reaction at equilibrium ? If not in which direction does the reaction tend to proceed to reach equilibrium ?

Equilibrium constant, K_(C ) for the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g) at 500 K is 0.061 At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^(-1)N_(2), 2.0 "mol L"^(-1) H_(2) , 0.5 mol L^(-1) NH_(3) . Is the reaction at equilibrium ? If not, in which direction does the reaction tends to proceed to reach equilibirum ?

Equilibrium constant, K_(c) for the reaction, N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g) at 500K is 0.061. at a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol*L^(-1)" "N_(2),2.0mol*L^(-1)" "H_(2) and 0.5mol*L^(-1)NH_(3) . is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium ?

Equilibrium constant 'K_c' for the reaction 'N_2(g)+3 H_2(g) hArr 2 N H_3(g)' at '500 K' is '0.061' At a particular time, the analysis shows that composition of the reaction mixture is '3.0 molL^(-1) N_2, 2.0' mol 'L^(-1) . H^2' and '0.5 mol L^(-1) NH_3 .' Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

Equilibrium constant, K_c for the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) _(at 500 k is 0.061) At a particular time, the analysis shows that composition of the reaction mixtue is 3.0 mol L^(-1) N_2,2.0 mol L^(-1) H_2 .5 mol L^(-1) NH_3 Is the eaction at equilibrium ?If not in which direction does the reaction tend to proceed to reach equilibrium?

At 500^(@)C the equilibrium constant for the reaction N_(2)(g) + 3H_(2) (g) hArr 2NH_(3)(g) is 6.02 xx 10^(-2) litre^(-2) mol^(-2) What is the value of K_(p) at the same temperature?