Chemical Equilibrium · Chemistry · AP EAPCET

At 500 K , for the reaction $$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$$, the $$K_p$$ is $$0.036 \mathrm{~atm}^{-2}$$. What is its $$K_C$$ in $$\mathrm{L}^2 \mathrm{~mol}^{-1}$$ ? $$\left(R=0.082 \mathrm{~L}^2\right.$$ atom $$\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$$.

The formation of ammonia from its constituent elements is an exothermic reaction. The effect of increased temperature on the reaction equilibrium is

At $$60^{\circ} \mathrm{C}$$, dinitrogen tetroxide is dissociated. Find it's standard free energy change at this temperature and one atmosphere. [Given $$\log 1.33=0.1239$$]

Le-Chatelier's principle is not applicable to

Using the data provided, find the value of equilibrium constant for the following reaction at $$298 \mathrm{~K}$$ and $$1 \mathrm{~atm}$$ pressure.

$$\begin{aligned} \mathrm{NO}(g)+\frac{1}{2} \mathrm{O}_2(g) \rightleftharpoons & \mathrm{NO}_2(g) \\ \Delta_f H \mathrm{Y}[\mathrm{NO}(g)] & =90.4 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \Delta_f H \mathrm{Y}\left[\mathrm{NO}_2(g)\right] & =32.48 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \Delta S Y a t ~298 \mathrm{~K} & =-70.8 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1} \end{aligned}$$

$$[\operatorname{antilog}(0.50)=3162 \text { ] }$$

Standard entropies of $$X_2, Y_2$$ and $$X Y_3$$ are 60, 40 and $$50 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$$ respectively. At what temperature, the following reaction will be at equilibrium? [given: $$\Delta H \Upsilon=-30 \mathrm{~kJ}$$]

$$\frac{1}{2} X_2+\frac{3}{2} Y_2 \rightleftharpoons X Y_3$$

For the reaction $$\mathrm{SO}_2(g)+\frac{1}{2} \mathrm{O}_2(g) \rightleftharpoons \mathrm{SO}_3(g)$$, the percentage yield of product at different pressure is shown in the figure. Then, which among the following is true?

Which among the following denotes the correct relationship between $$K_p$$ and $$K_c$$ for the reaction, $$2 A(g) \rightleftharpoons B(g)+C(g)$$