Relation between Kp and Kc

Q. For the synthesis of ammonia, $K_p$ and $K_c$ are related as:

1. $K_p=K_c(RT{)}^2$
2. $K_c=K_p(RT{)}^{-2}$
3. $K_c=K_p(RT{)}^2$
4. $K_p=K_c$

Q.

For a general reaction aA(g) + bB(g) $\leftrightharpoons$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_c$ and $K_p$? [assume $\Delta$n = $\mu$ = (c + d) - (a+b) ]\)

1. =

2. =

3. = 1

4. =

Q.

In which of the following equilibria, the value of $K_P$ is less than $K_C$

1. H₂ + I₂ 2HI

2. N₂ + 3H₂ 2NH₃

3. N₂ + O₂ ​ 2NO

4. CO + H₂O CO₂ + H₂

Q.

0.96g of HI were heated to attain equilibrium

$2HI\rightleftharpoons H2+I2$. The reaction mixture on titration requires 15.7ml of $\frac{N}{10}$ hypo. Calculate % dissociation of HI.

1. 18.9%

2. 19.9%

3. 20.9%

4. 21.9%

Q.

For $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)+heat$

1. K_P = K_C (RT)²

2. K_P = K_C (RT)

3. K_P = K_C (RT)^-2

4. K_P = K_C (RT)^-1

Q. For a given exothermic reaction, $K_p$ and $K_p^{\prime }$ are the equilibrium constants at temperatures $T_1$ and $T_2$ respectively. Assuming that heat of reaction is constant in temperatures range between $T_1$ and $T_2$. It is readily observation that :
(Given, $T_2>T_1$)

1. $K_P>K_P^{\prime }$
2. $K_P<K_P^{\prime }$
3. $K_P=K_P^{\prime }$
4. $K_{=}\frac{1}{K_P^{\prime }}$

Q.

For the reaction $PC{l}_3\left(g\right)+C{l}_2\left(g\right)\rightleftharpoons PC{l}_5\left(g\right)$ at ${2500}^{\circ }C$, the value of $K_C$ is $26$, then the value of $K_P$ at the same temperature will be

1. 0.61

2. 0.57

3. 0.83

4. 0.46

Q. At ${800}^{\circ }$C, the following equilibrium is established as
$F_2\left(g\right)\rightleftharpoons 2F\left(g\right)$
The composition of equilibrium may be determined by measuring the rate of effusion of the mixture through a pin hole. It is found that at ${800}^{\circ }$C and 1 atm mixture effuses 1.6 times as fast as $S{O}_2$ effuses under the similar conditions. (Atomic weight of F =19 amu). What is the value of $K_p$?

1. 0.315 atm
2. 0.685 atm
3. 0.460 atm
4. 1.490 atm

Q.

In the reaction

$C{S}_2\left(l\right)+3O_2\left(g\right)\to C{O}_2\left(g\right)+2S{O}_2\left(g\right)\Delta H=-265kcal$

The enthalpies of formation of $C{O}_2$ and $S{O}_2$ are both negative and are in the ratio 4 : 3. The enthalpy of formation of $C{S}_2$ is $+26kcal/mol$. Calculate the enthalpy of formation of $S{O}_2$.

1. −52 kcal/mol

2. −90 kcal/mol

3. −78 kcal/mol

4. −71.7 kcal/mol

Q. Two solid compounds ${}^{\prime }{X}^{\prime }$ and ${}^{\prime }{Y}^{\prime }$ dissociates at certain temperature as follows:
$X\left(s\right)\rightleftharpoons A\left(g\right)+2b\left(g\right)K{p}_1=9\times {10}^{-3}{\text{atm}}^3$
$Y\left(s\right)\rightleftharpoons 2B\left(g\right)+C\left(g\right)K{p}_2=4.5\times {10}^{-3}{\text{atm}}^3$.
The total pressure (in atm) of gases over a mixture of ${}^{\prime }{X}^{\prime }$ and ${}^{\prime }{Y}^{\prime }$ is

1. 1.5
2. 0.45
3. 0.6
4. 0.9

Q. Solid ammonium carbamate, $N{H}_{4}C{O}_{2}N{H}_2\left(s\right)$, dissociates into ammonia and carbon dioxide when it evaporates as shown by
$N{H}_{4}C{O}_{2}N{H}_2\left(s\right)\rightleftharpoons 2N{H}_3\left(g\right)+C{O}_2\left(g\right)$
At ${25}^{\circ }C$, the total pressure of the gases in equilibrium with the solid is $0.116\text{atm}$, if $0.1\text{atm}$ of $C{O}_2$ is introduced after equilibrium is reached then:

1. The final pressure of $C{O}_2$ will be less than $0.1\text{atm}$
2. The final pressure of $C{O}_2$ will be more than $0.1\text{atm}$
3. The pressure of $N{H}_3$ will decrease due to addition of $C{O}_2$
4. The pressure of $N{H}_3$ will increase due to addition of $C{O}_2$

Q.

For which one of the following homogenous equilibrium equations will K_p equal K_c?

1. 3H₂ (g) + N₂ (g) ⇌ 2NH₃ (g)

2. PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g)

3. COCl₂ (g) ⇌ CO (g) + Cl₂ (g)

4. H₂ (g) + I₂ (g) ⇌ 2HI (g)

Q. At 700 K, the equilibrium constant $K_p,$ for the reaction
$2S{O}_3\left(g\right)\rightleftharpoons 2S{O}_2\left(g\right)+O_2\left(g\right)$
is $1.8\times {10}^{-3}kPa.$ What is the numerical value of $K_C$ for this reaction at the same temperature?
$R=0.0821Latmmo{l}^{-1}{K}^{-1}$

1. $3.09\times {10}^{-7}molelitr{e}^{-1}$
2. $9.03\times {10}^{-7}molelitr{e}^{-1}$
3. $5.05\times {10}^{-9}molelitr{e}^{-1}$
4. $5.05\times {10}^{-5}molelitr{e}^{-1}$

Q. $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ is a gaseous phase equilibrium reaction taking place in a $5$ litre flask at $1atm$. For this :

1. $K_C=K_p$
2. $K_C=25K_p$
3. $K_p=25K_c$
4. $K_C=5K_p$

Q.

The ratio of $K_p$ to $K_c$ for the equilibrium $CO\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\rightleftharpoons C{O}_2\left(g\right)$ is

1. 1

2. RT

3. $\frac{1}{\sqrt{RT}}$

4. $(RT{)}^{\frac{1}{2}}$

Q. For the synthesis of ammonia, $K_p$ and $K_c$ are related as:

1. $K_p=K_c(RT{)}^2$
2. $K_c=K_p(RT{)}^{-2}$
3. $K_c=K_p(RT{)}^2$
4. $K_p=K_c$

Q.

For $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)+heat$

1. $K_P=K_C(RT{)}^2$

2. $K_P=K_C\left(RT\right)$

3. $K_P=K_C(RT{)}^{-2}$

4. $K_P=K_C(RT{)}^{-1}$