A mixture of 1.57 mol of `N_2`, 1.92 mol of `H_2` and 8.13 mol of `NH_3` is introduced into a 20L vessel at 500K. `K_c` for the reaction `N_2+3H_2iff2NH_3` is `1.7 xx10^2` at 500K. Is the reaction mixture at equilibrium. If not, what is the direction of the net reaction.

The graph showing the progress of the reaction N_2+3H_2harr2NH_3 , is given What is the significance of the state A?

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?

The K_(c) of the hypothetical reaction P+Q iff R+S is 3 times 10^(-1) at 400 K and 2 times 10^(-2) at 500 K. From this data, one can infer that, for the reaction

The enthalpy change for the reaction, N_2(g)+3H_2(g)rightarrow2NH_3(g) Is -92.38 kJ at 298 K. What is DeltaU at 298 K?

N_2 + 3H_2 harr 2NH_3 + Heat What is the effect of increasing temperature on value of K?

If the K_(c) of the reaction N_(2)(g)+3H_(2)(g) iff 2NH_(3)(g) at 750 K is 49, then the K_(c) of the reaction NH_(3)(g) iff 1/2N_(2)(g)+3/2H_(2)(g) at the same temperature is

The specific reaction rate of a reaction is 6.2 x10^(-3) (mol) (L)^(-1) (s)^(-1) . What is the order of the reaction?