Question

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Answer 1

Correct  Question:

In a 500 mL capacity vessel, CO and Cl₂are mixed to form COCl₂

At equilibrium, it contains 0.2 moles of COCI,

and 0.1 moles of each of CO and Cl₂.The equilibrium constant K for reaction, CO +

C1₂ →COCI₂ is:

Given:

The volume of the solution = 500 ml = 0.5 L

Moles of reactants and products present at equilibrium:

CO = Cl₂ = 0.1 moles

COCl₂ = 0.2 moles

To find:

Equilibrium constant

Formula:

For a given reaction ,

aA + bB $\rightleftharpoons$ cC + dD

The equilibrium constant is given by,

$\to \sf{K_c= \dfrac{[C]^c .[D]^d}{[A]^a.[B]^b}}$

K꜀ = equilibrium constants

a,b,c,d = stotiometric coefficients

A,B,C,D = concentration in mol/L

Solution:

Given reaction,

CO +

C1₂ $\rightleftharpoons$ COCI₂

The equilibrium constant is given by,

$\to \sf{K_c= \dfrac{[COCl_2]}{[CO].[Cl_2]}}$

Here,

[COCI₂] = 0.2/0.5 = 0.4

[CO] = [Cl₂] = 0.1/0.5 = 0.2

Now let's substitute these values in the above equation,

$\to \sf{K_c= \dfrac{0.4}{0.2 \times 0.2}}$

$\to \sf{K_c= \dfrac{0.4}{0.04}}$

$\to \sf{K_c= 10}$

The equilibrium constant for the reaction is 10.

Answer 2

Correct Question:

In a 500 mL capacity vessel, CO and Cl₂are mixed to form COCl₂

At equilibrium, it contains 0.2 moles of COCI,

and 0.1 moles of each of CO and Cl₂.The equilibrium constant K for reaction, CO +

C1₂ →COCI₂ is:

Given:

The volume of the solution = 500 ml = 0.5 L

Moles of reactants and products present at equilibrium:

CO = Cl₂ = 0.1 moles

COCl₂ = 0.2 moles

To find:

Equilibrium constant

Formula:

For a given reaction ,

aA + bB \rightleftharpoons⇌ cC + dD

The equilibrium constant is given by,

\begin{gathered}\to \sf{K_c= \dfrac{[C]^c .[D]^d}{[A]^a.[B]^b}}\\ \\\end{gathered}

→K

c

=

[A]

a

.[B]

b

[C]

c

.[D]

d

K꜀ = equilibrium constants

a,b,c,d = stotiometric coefficients

A,B,C,D = concentration in mol/L

Solution:

Given reaction,

CO +

C1₂ \rightleftharpoons⇌ COCI₂

The equilibrium constant is given by,

\begin{gathered}\to \sf{K_c= \dfrac{[COCl_2]}{[CO].[Cl_2]}}\\ \\\end{gathered}

→K

c

=

[CO].[Cl

2

]

[COCl

2

]

Here,

[COCI₂] = 0.2/0.5 = 0.4

[CO] = [Cl₂] = 0.1/0.5 = 0.2

Now let's substitute these values in the above equation,

\begin{gathered}\to \sf{K_c= \dfrac{0.4}{0.2 \times 0.2}}\\ \\\end{gathered}

→K

c

=

0.2×0.2

0.4

\begin{gathered}\to \sf{K_c= \dfrac{0.4}{0.04}}\\ \\\end{gathered}

→K

c

=

0.04

0.4

\begin{gathered}\to \sf{K_c= 10}\\ \\\end{gathered}

→K

c

=10

The equilibrium constant for the reaction is 10.