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Standard XII

Chemistry

Characteristics of Chemical Equilibrium

If the pressu...

Question

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume, what will happen to the concentrations of $C O$ and ${C O}_{2}$ ?
$H_{2} O (g) + C O (g) ⇌ H_{2} (g) + {C O}_{2} (g) + H e a t$

both the [

C O

] and [

{C O}_{2}

] will decrease

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neither the [

C O

] nor the [

{C O}_{2}

] will change

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the [

C O

] will decrease and the [

{C O}_{2}

] will increase

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both the [

C O

] and [

{C O}_{2}

] will increase

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Solution

The correct option is C both the [ $C O$ ] and [ ${C O}_{2}$ ] will increase
Solution:- (D) both the $[C O]$ and $[C O_{2}]$ will increase
For the reaction-

${H_{2}}_{(g)} + {C O}_{(g)} ⇌ {H_{2}}_{(g)} + {C O_{2}}_{(g)} + Heat$

On decreasing the volume, the concentrations of both, i.e., reactants and products will increase.

Hence the both $[C O]$ and $[C O_{2}]$ will increase.

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Similar questions

Calculate $K_{c}$ for the equilibrium process, ${C O}_{2 (g)} + H_{2 (g)} ⇌ {C O}_{(g)} + H_{2} O_{(g)}$ . At equilibrium the reaction system contains 3.52 g of ${C O}_{2}$ , 1.4 g of $C O$ , 0.08 g of $H_{2}$ and 0.72 g of $H_{2} O$ .

(Atomic masses : $C = 12, H = 1, O = 16$ )

Write up to 3 decimal places.

Q. One mole of

H_{2} O

and one mole of

C O

are taken in 10 L vessel and heated to 725 K. At equilibrium, 40% of water (by mass) reacts with

C O

according to the equation.

H_{2} O (g) + C O (g) ⇌ H_{2} (g) + {C O}_{2} (g)

Calculate the equilibrium constant for the reaction.

Q. Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(i)

{C O C l}_{2} (g) ⇌ C O (g) + {C l}_{2} (g)

(ii)

{C H}_{4} (g) + 2 S_{2} (g) ⇌ {C S}_{2} (g) + 2 H_{2} S (g)

(iii)

{C O}_{2} (g) + C (s) ⇌ 2 C O (g)

(iv)

2 H_{2} (g) + C O (g) ⇌ {C H}_{3} O H (g)

(v)

{C a C O}_{3} (s) ⇌ C a O (s) + {C O}_{2} (g)

(vi)

4 {N H}_{3} (g) + 5 O_{2} (g) ⇌ 4 N O (g) + 6 H_{2} O (g)

Q. Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
(a)

{P C l}_{5} (g) ⇌ {P C l}_{3} (g) {C l}_{2} (g)

(b)

C a O (s) + {C O}_{2} (g) ⇌ {C a C O}_{3} (s)

(c)

3 F e (s) + 4 H_{2} O (g) ⇌ {F e}_{3} O_{4} (s) + 4 H_{2} (g)

Q. An equilibrium mixture of

C O (g) + H_{2} O (g) ⇋ C O_{2} (g) + H_{2} (g)

, present in a vessel of one litre capacity at

815^{\circ} C

was found by analysis to contain 0.4 mole of CO, 0.3 mole of

H_{2} O

, 0.2 mole of

C O_{2}

and 0.6 mole of

H_{2}

(a) Calculate

K_{c}

.
(b) If it is derived to increase the concentration of CO to 0.6 moles by adding

C O_{2}

to the vessel, how many moles must be added into equilibrium mixture at a constant temperature in order to get this change?

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If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume, what will happen to the concentrations of CO and CO2? H2O(g)+CO(g)⇌H2(g)+CO2(g)+Heat

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume, what will happen to the concentrations of $C O$ and ${C O}_{2}$ ?
$H_{2} O (g) + C O (g) ⇌ H_{2} (g) + {C O}_{2} (g) + H e a t$