For the given equilibrium reaction,2 A(g) rig | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$.Here,$\Delta n = (2 + 1) - 2 = 1$.Given $T = 800 \ K

Vedclass · Accepted Answer

$0.026$

Vedclass · Answer

(B) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$.Here,$\Delta n = (2 + 1) - 2 = 1$.Given $T = 800 \ K$ and $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$.Note: The value of $K_c$ changes with temperature. However,assuming the provided $K_c$ value is intended for the calculation at $800 \ K$ (as is common in such textbook problems),we use $K_c = 4 	imes 10^{-4}$.$K_p = (4 	imes 10^{-4}) 	imes (0.082 	imes 800)^1$.$K_p = 0.0004 	imes 65.6 = 0.02624 \approx 0.026$.

For the given equilibrium reaction,$2 A(g) \rightleftharpoons 2 B(g) + C(g)$,the equilibrium constant $(K_c)$ at $1000 \ K$ is $4 \times 10^{-4}$. Calculate $K_p$ for the reaction at $800 \ K$ temperature.

Similar Questions

The reaction between $N_2$ and $H_2$ to form ammonia has $K_c = 6 \times 10^{-2}$ at the temperature $500 \ ^oC$. The numerical value of $K_p$ for this reaction is

If the degree of dissociation is $\sqrt{0.5}$,what will be the value of $K_p$ for the reaction $N_2O_3 \rightleftharpoons NO + NO_2$ in terms of the total pressure $P$?

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,$K_C$ at $427\ ^oC$ is $3 \times 10^{-6}\ mol\ L^{-1}$. The value of $K_P$ is nearly $....... \times 10^{-4}$.

For the reaction $CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$,$\frac{K_p}{K_c}$ is equal to

Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$
$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$
Which of the following relations is correct?

Vedclass Test Series

Exam Paper Generator

Online Exam Module