Consider the following reaction:

$2 S O_{2} (g) + O_{2} (g) ⇋ 2 S O_{3} (g) + h e a t$

If we increase the temperature of the given equilibrium system then an exothermic reaction will be favoured.

True

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False

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Solution

The correct option is B
False

When the temperature of the reaction is increased, then, according to Le Chatelier's principle the equilibrium system will try to readjust itself to counteract this effect. If we increase the temperature then the system will try to reduce it. Therefore, an endothermic reaction will occur favoring a forward reaction. As a result, sulphur trioxide will be formed from sulphur dioxide and oxygen.

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Similar questions

K_{p} = 2.0 \times 10^{10}

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

K_{c}

Consider the following reaction:

$2 S O_{2} (g) + O_{2} (g) ⇋ 2 S O_{3} (g) + h e a t$

If we increase the temperature of the given equilibrium system then an exothermic reaction will be favoured.

Consider the following reaction:

$2 S O_{2} (g) + O_{2} (g) ⇋ 2 S O_{3} (g) + h e a t$

What will happen if the temperature of the reacting system is decreased?

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

S O_{2}

O_{2}

S O_{3}

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

S O_{3}

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