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Introduction to Le Chatelier's Principle

Consider the ...

Question

Consider the reactions given below. In which cases will the reaction proceed toward right by increasing the pressure?

4 H C l (g) + O_{2} (g) ⟶ 2 {C l}_{2} (g) + 2 H_{2} O (g)

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{C l}_{2} (g) + H_{2} O (g) ⟶ 2 H C l (g) + \frac{1}{2} O_{2} (g)

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{C O}_{2} (g) + 4 H_{2} (g) ⟶ {C H}_{4} (g) + 2 H_{2} O (g)

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O_{2} (g) + O_{2} (g) ⟶ 2 N O (g)

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Solution

The correct options are
A $4 H C l (g) + O_{2} (g) ⟶ 2 {C l}_{2} (g) + 2 H_{2} O (g)$
C ${C O}_{2} (g) + 4 H_{2} (g) ⟶ {C H}_{4} (g) + 2 H_{2} O (g)$

Suggest Corrections

Similar questions

Δ_{r} U^{\circ}

4 H C l (g) + O_{2} (g) \to 2 C l_{2} (g) + 2 H_{2} O (g)

H_{2} (g) + C l_{2} (g) \to 2 H C l (g)

Δ_{r} H_{300}^{^{\circ}} = - 184.5 k J / m o l

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (g)

Δ_{r} H_{300}^{^{\circ}} = - 483 k J / m o l

Which of the following reactions is not correct according to the law of conservation of mass ?

(a) $2 M g (s) + O_{2} (g) \to 2 M g O (s)$

(b) $C_{3} H_{8} (g) + O_{2} (g) \to C O_{2} (g) + H_{2} O (g)$

(d) $C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g)$

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g) + 800 k J

O_{2} (g)

2 C l_{2} (g) + 2 H_{2} O (g) ⇌ 4 H C l (g) + O_{2} (g)

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

H C l

Δ_{f} U

4 H C l (g) + O_{2} (g) ⇌ 2 {C l}_{2} (g) + 2 H_{2} O (g)

H_{2} (g) + {C l}_{2} (g) ⟶ 2 H C l (g) Δ_{f} H_{300} = - 184.5 k J / m o l e

H_{2} (g) + O_{2} (g) ⟶ {2 H}_{2} O (g) Δ_{f} H_{300} = - 483 k J / m o l e (U s e R = 8.3 J / m o l e)

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