For which of the following reactions will {K_ | vedclass

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

Question

(C) The relationship between ${K_p}$ and ${K_c}$ is given by the equation: ${K_p} = {K_c}{(RT)^{\Delta n_g}}$.For ${K_p} > {K_c}$,the value of ${\Delt

Vedclass · Accepted Answer

${PCl_{5(g)}} \rightleftharpoons {PCl_{3(g)}} + {Cl_{2(g)}}$

Vedclass · Answer

(C) The relationship between ${K_p}$ and ${K_c}$ is given by the equation: ${K_p} = {K_c}{(RT)^{\Delta n_g}}$.For ${K_p} > {K_c}$,the value of ${\Delta n_g}$ must be positive $({\Delta n_g} > 0)$.${\Delta n_g}$ is the difference between the number of moles of gaseous products and gaseous reactants.For option $A$: ${\Delta n_g} = 2 - (1 + 3) = -2$.For option $B$: ${\Delta n_g} = 2 - (1 + 1) = 0$.For option $C$: ${\Delta n_g} = (1 + 1) - 1 = +1$.For option $D$: ${\Delta n_g} = 2 - (2 + 1) = -1$.Since ${\Delta n_g} > 0$ only for option $C$,the correct answer is $C$.

For which of the following reactions will ${K_p} > {K_c}$?

Similar Questions

At $300 \ K$,$K_C$ for the reaction $A_2B_{2(g)} \rightleftharpoons A_{2(g)} + B_{2(g)}$ is $100 \ mol \ L^{-1}$. What is its $K_p$ (in $atm$) at the same temperature? $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

For the reaction, $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $300 \ K$, the value of $\Delta G^{\circ}$ is $-690.9 R$. The equilibrium constant value for the reaction at that temperature is ($R$ is gas constant).

$A$ sample of $HI_{(g)}$ is placed in a flask at a pressure of $0.2 \ atm$. At equilibrium,the partial pressure of $HI_{(g)}$ is $0.04 \ atm$. What is $K_{p}$ for the given equilibrium?
$2 HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$

The partial pressures of $CH_3OH$,$CO$ and $H_2$ in the equilibrium mixture for the reaction $CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)$ at $427 \ ^oC$ are $2.0 \ atm$,$1.0 \ atm$ and $0.1 \ atm$ respectively. The value of $K_P$ for the decomposition of $CH_3OH$ to $CO$ and $H_2$ is:

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

Vedclass Test Series

Exam Paper Generator

Online Exam Module