Calculate the value of Q c value- for the given reaction below- Also- given the concentration of all the species involved at a certain time- CO - g - H - 2 O - g rightleftharpoons CO - 2 - g - H - 2 - g - CO - 2-2 - M - H - 2-2 - M - CO -1 - M - H - 2 O -1 - M -If K c -1- in which direction the reaction will shift to attain equilibrium-A- Q C -2 and backwardB- Q C -4 and forwardC- Q C -4 and backwardD- Q C -2 and forward

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Reaction Quotient

Calculate the...

Question

Calculate the value of $Q_{c}$ value, for the given reaction below. Also, given the concentration of all the species involved at a certain time:
$C O (g) + H_{2} O (g) ⇌ C O_{2} (g) + H_{2} (g) [C O_{2}] = 2 M [H_{2}] = 2 M [C O] = 1 M [H_{2} O] = 1 M$

If $K_{c} = 1$ , in which direction the reaction will shift to attain equilibrium?

Q_{C} = 2

and forward

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Q_{C} = 2

and backward

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Q_{C} = 4

and forward

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Q_{C} = 4

and backward

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Solution

The correct option is D $Q_{C} = 4$ and backward
We know for a reaction:
$a A (g) + b B (g) ⇌ c C (g) + d D (g)$
In terms of Concentration :
$Q_{c} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}$

So, In this case,
$Q_{c} = \frac{[C O_{2}] . [H_{2}]}{[C O] . [H_{2} O]} = \frac{2 \times 2}{1 \times 1} = 4$
Comparing $Q_{c} a n d K_{c}$
Since, $Q_{c} > K_{c}$ the reaction shifts backwards (to the reactants side) for attaining equilibrium.

Theory:
Reaction quotient :
The reaction quotient (Q) measures the relative amounts of products and reactants present during a reaction at a particular point in time.
Reaction :
$a A (g) + b B (g) ⇌ c C (g) + d D (g)$
In terms of Partial Pressure :
$Q_{p} = \frac{[P]_{c}^{c} [P]_{d}^{d}}{[P]_{a}^{a} [P]_{b}^{b}}$
In terms of Concentration :
$Q_{c} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}$

Applications of Reaction quotient :
Case 1 :-
$Q_{c} > K_{c}$
For the given reaction :
$R ⇌ P$

If $Q_{c} > K_{c}$ or if $Q_{c} \neq K_{c}$ this means that system is not in equilibrium.
$Q_{c}$ will move close toward $K_{c}$ until it becomes equal to $K_{c}$ .
Value of $K_{c}$ (equilibrium constant) remains constant.
It promotes backward reaction when $Q_{c} > K_{c}$ to attain equilibrium.

Case 2 :- $Q_{c} < K_{c}$
For the given reaction :
$R ⇌ P$

If $Q_{c} < K_{c}$ or if $Q_{c} \neq K_{c}$ this means that system is not in equilibrium.
$Q_{c}$ will move close toward $K_{c}$ until it becomes equal to $K_{c}$ . It promotes forward reaction when $Q_{c} < K_{c}$ to attain equilibrium.

Suggest Corrections

Similar questions

Q. Calculate the value of

Q_{c}

value, for the given reaction below. Also, given the concentration of all the species involved at a certain time:

C O (g) + H_{2} O (g) ⇌ C O_{2} (g) + H_{2} (g) [C O_{2}] = 2 M [H_{2}] = 2 M [C O] = 1 M [H_{2} O] = 1 M

K_{c} = 1

, in which direction the reaction will shift to attain equilibrium?

Q. The value of Kc = 4.24 at 800 Kfor the reaction CO(g) + H2O (g) gives rise to CO2(g) + H2(g) Calculate equilibrium concentrations of CO2, H2, CO and H2O at 800 K , if only CO and H2O are present initially at concentration of 0.10 M each ?

Q. The value of

K_{c} = 4.24

800 K

for the reaction

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

Calculate equilibrium concentrations of

{C O}_{2}, H_{2}, C O

and

H_{2} O

800 K

, if only

C O

and

H_{2} O

are present initially at concentration of

0.10 M

each.

Q. For the reaction,

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

the value of Kc at

552^{\circ} C

is 0.137. If 5 moles of

{C O}_{2}

, 5 moles of

H_{2}

, 1 mole of

C O

and 1 mole of

H_{2} O

are initially present what are the actual concentrations of

{C O}_{2}, H_{2}, C O, H_{2} O

at equilibrium?

Q. The standard enthalpy and entropy changes for the reaction in equilibrium for the forward direction are given below:

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

Δ H_{300 K}^{o} = - 41.16 k J {m o l}^{- 1}

Δ S_{300 K}^{o} = - 4.24 \times 10^{- 2} k J {m o l}^{- 1}

Δ H_{1200 K}^{o} = - 32.93 k J {m o l}^{- 1}

Δ S_{1200 K}^{o} = - 2.96 \times 10^{- 2} k J {m o l}^{- 1}

Calculate

K_{P}

at each temperature and predict the direction of reaction at

300 K

and

1200 K

, when

P_{C O} = P_{{C O}_{2}} = P_{H_{2}} = P_{H_{2} O} = 1

atm at initial state.

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Reaction Quotient

Standard XII Chemistry

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Calculate the value of Qc value, for the given reaction below. Also, given the concentration of all the species involved at a certain time: CO (g)+H2O (g)⇌CO2 (g)+H2 (g)[CO2]=2 M[H2]=2 M[CO]=1 M[H2O]=1 M If Kc=1 , in which direction the reaction will shift to attain equilibrium?