In a chemical reaction,the rate constant for the backward reaction is $7.5 \times 10^{-4}$ and the equilibrium constant is $1.5$. The rate constant for the forward reaction will be .......

The standard equilibrium constant,$K_p$ at $298 \, K$ for the reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ is $5.8 \times 10^5$. The value of standard equilibrium constant,if the concentration of gases is expressed in terms of $mol/L$,will be:
[Given : $R = 0.08314 \, L \, bar \, K^{-1} \, mol^{-1}$]

$A$ schematic plot of $\ln K_{eq}$ versus inverse of temperature $(1/T)$ for a reaction is shown below. The reaction must be

For the reaction $P + Q \rightleftharpoons R + C$,the equilibrium constant $K_c$ is $10^{-2}$ and the forward rate constant $K_f$ is $10^{-1}$. The rate constant for the backward reaction $(K_b)$ will be:

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $25^o C$,the value of $K_c$ is $6.10 \times 10^{-3}$. What is the value of $K_c$ for the equilibrium reaction $NO_{2(g)} \rightleftharpoons 1/2 N_2O_{4(g)}$?

For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $\frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{(g)}$,if the equilibrium constants are $K_1$ and $K_2$ respectively,then their relationship is: