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Standard XII

Chemistry

Derivation of Kp and Kc

The equilibri...

Question

The equilibrium constant for the reaction: $2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}$ is 5. If the equilibrium constant mixture contains equal moles of $S O_{3}$ and $S O_{2}$ , the equilibrium partial pressure of $O_{2}$ gas is:

0.2 atm

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2 atm

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0.02 atm

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0.04 atm

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Solution

The correct option is B 0.2 atm
$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$
$P_{S O_{3}} = P_{S O_{2}}$
$K_{p} = \frac{(P_{S O_{3}})^{2}}{(P_{S O_{2}})^{2} P_{O_{2}}} = 5$
$= \frac{1}{P_{O_{2}}} = 5$
$P_{O_{2}} = \frac{1}{5} = 0.2$

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Similar questions

Q. The equilibrium constant

K_{p}

for the reaction

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

1000 K

is 3.5. What would be the partial pressure of

O_{2}

gas with equal moles of

S O_{2}

and

S O_{3}

at equilibrium?

Q. The equilibrium constant

K_{p}

of the reaction:

2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)

is 900 atm at 800 K. A mixture containing

S O_{3}

and

O_{2}

having initial partial pressure of 1 and 2 atm. respectively is heated at constant volume to equilibriate. Calculate the partial pressure of

O_{2}

gas at 800 K.

Q. At T(K), the partial pressures of

S O_{2}, O_{2}

and

S O_{3}

are 0.662, 0.100 and 0.331 atm, respectively for the reaction

{2 S O_{2}}_{(g)} + {O_{2}}_{(g)} ⇌ {2 S O_{3}}_{(g)}

at equilibrium. What is the partial pressure in atm, of

O_{2}

when the equilibrium partial pressures of

S O_{2}

and

S O_{3}

are equal at the same temperature ?

Q. The

K_{p}

for

2 S O_{2 (g) + O_{2 (g)}} ⇌ 2 S O_{3 (g)}

5.0 a t m^{- 1}

.What is the equilibrium partial pressure of

O_{2}

if the equilibrium pressure of

S O_{2}

and

S O_{3}

are equal?

The equilibrium constant Kp of the reaction, 2 $S O_{2}$ (g) + $O_{2}$ (g) $\leftrightharpoons$ 2 $S O_{3}$ (g) is 900 atm. at 800 K. A mixture containing $S O_{3}$ and $O_{2}$ having initial pressure of 1 and 2 atm respectively is heated at constant volume to equilibrate. Calculate the partial pressure of $S O_{2}$ gas at 800 K.

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The equilibrium constant for the reaction: 2SO2(g)+O2(g)⇌2SO3(g) is 5. If the equilibrium constant mixture contains equal moles of SO3 and SO2, the equilibrium partial pressure of O2 gas is:

The correct option is B 0.2 atm2SO2+O2⇌2SO3PSO3=PSO2Kp=(PSO3)2(PSO2)2PO2=5=1PO2=5PO2=15=0.2

The equilibrium constant for the reaction: $2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}$ is 5. If the equilibrium constant mixture contains equal moles of $S O_{3}$ and $S O_{2}$ , the equilibrium partial pressure of $O_{2}$ gas is:

The correct option is B 0.2 atm
$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$
$P_{S O_{3}} = P_{S O_{2}}$
$K_{p} = \frac{(P_{S O_{3}})^{2}}{(P_{S O_{2}})^{2} P_{O_{2}}} = 5$
$= \frac{1}{P_{O_{2}}} = 5$
$P_{O_{2}} = \frac{1}{5} = 0.2$