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Characteristics of Equilibrium Constant

For the gas p...

Question

For the gas phase reaction (1) shown below, which of the following statement is true for reaction (2)?
1. $2 N O ⇌ N_{2} + O_{2}, Δ H = - 43.5 k C a l$
2. $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$

A

K

is independent of

T

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B

K

decreases as

T

decreases

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C

K

increases as

T

decrease

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D

K

varies with addition of

N O

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Solution

The correct option is B $K$ decreases as $T$ decreases
For the second endothermic reaction (because the reverse reaction is endothermic), $K$ decreases as $T$ decreases by Le-Chatelier's Principle.

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Similar questions

Q. For the gas phase reaction,

2 N O ⇌ N_{2} + O_{2}; Δ H = - 43.5 k c a l

Which of the following is/are true of

N_{2} + O_{2} ⇌ 2 N O ?

Q. For the gas phase reaction

2 N O \Leftrightarrow N_{2} + O_{2}, Δ H = - 43.5 k c a l s

. Which one of the following is true for the reaction?

Q. The variation of K and

K_{f}

K_{b}

with temperature shows the following effects:
(i) For endothermic reaction K increases and

K_{f}

K_{b}

also increases with temperature.
(ii) For endothermic reaction K decreases and

K_{f}

K_{b}

also decreases with temperature.
(iii) For exothermic reaction K decreases and

K_{f}

K_{b}

both increases with temperature.
(iv) For exothermic reaction K increases and

K_{f}

K_{b}

decreases with temperature.
(v) For exothermic reaction K decreases and

K_{f}

K_{b}

both decreases with temperature.

Q. Assertion :Observed rate constant of the given reaction given below decreases with temperature.

N O + N O_{f} K_{b} N_{2} O_{2}

N_{2} O_{2} + O_{2} K \to s l o w 2 N O_{2}

2 N O + O_{2} \to 2 N O_{2}

K_{c}

of the reaction being exothermic and decrease in

K_{c}

overweigh increase in K with increase in temperature.

K_{c} = 7.5 \times 10^{- 9}

at 1000 K for the reaction

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

K_{c}

at 1000 K for the reaction

2 N O (g) ⇌ N_{2} (g) + O_{2} (g)

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