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Byju's Answer

Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

Listed in the...

Question

Listed in the table are forward and reverse rate constants for the reaction $2 N O (g) ⇌ N_{2} (g) + O_{2} (g)$ .

Temperature (K)
$k_{f} (M^{- 1} s^{- 1})$
$k_{r} (M^{- 1} s^{- 1})$
1400
0.29
$1.1 \times 10^{- 6}$
1500
1.3
$1.4 \times 10^{- 5}$

Is the reaction endothermic or exothermic?

Exothermic reaction

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Endothermic reaction

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Can't predict

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None of these

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Solution

The correct option is A Exothermic reaction
At 1400 K,

$K = \frac{K_{f}}{K_{r}} = \frac{0.29}{1.1 \times 10^{- 6}} = 2.64 \times 10^{5}$

At 1500 K,

$K = \frac{K_{f}}{K_{r}} = \frac{1.3}{1.4 \times 10^{- 5}} = 9.29 \times 10^{4}$
Thus, with an increase in temperature, the value of the equilibrium constant decreases. Hence, the reaction is exothermic.

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Similar questions

Q. Listed in the table are forward and reverse rate constants for the reaction

2 N O (g) ⇌ N_{2} (g) + O_{2} (g)

\begin{matrix} T e m p e r a t u r e (K) & K_{f} (M^{- 1} s^{- 1}) & k_{r} (M^{- 1} s^{- 1}) 1400 & 0.29 & 1.1 \times 10^{- 6} 1500 & 1.3 & 1.4 \times 10^{- 5} \end{matrix}

Is the reaction endothermic or exothermic?

Q. If

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

at 1000 K for the reaction

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

, what is

K_{c}

at 1000 K for the reaction

2 N O (g) ⇌ N_{2} (g) + O_{2} (g)

Q. For the reaction

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g,)

the equilibrium constant is

K_{1} .

The equilibrium constant is

K_{2}

for the reaction

2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g) .

What is

K

for the reaction

N O_{2} (g) ⇌ \frac{1}{2} N_{2} (g) + O_{2} (g)

Q. For the reaction,

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

, the equilibrium constant is

K_{1}

. The equilibrium constant is

K_{2}

for the reaction,

2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g)

What is

K

for the reaction,

N O_{2} (g) ⇌ \frac{1}{2} N_{2} (g) + O_{2} (g)

Q. The equilibrium constant (

K_{c}

) for the reaction,

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

at temperature (

T

) is

4 \times 10^{- 4}

. The value of

K_{c}

for the reaction,

N O (g) ⇌ \frac{1}{2} N_{2} (g) + O_{2} (g)

at the same temperature is:

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Temperature (K)	$k_{f} (M^{- 1} s^{- 1})$	$k_{r} (M^{- 1} s^{- 1})$
1400	0.29	$1.1 \times 10^{- 6}$
1500	1.3	$1.4 \times 10^{- 5}$

Listed in the table are forward and reverse rate constants for the reaction 2NO(g)⇌N2(g)+O2(g).Temperature (K)kf(M−1s−1)kr(M−1s−1)14000.291.1×10−615001.31.4×10−5Is the reaction endothermic or exothermic?

The correct option is A Exothermic reactionAt 1400 K,K=KfKr=0.291.1×10−6=2.64×105At 1500 K,K=KfKr=1.31.4×10−5=9.29×104Thus, with an increase in temperature, the value of the equilibrium constant decreases. Hence, the reaction is exothermic.

Listed in the table are forward and reverse rate constants for the reaction $2 N O (g) ⇌ N_{2} (g) + O_{2} (g)$ .

Temperature (K)
$k_{f} (M^{- 1} s^{- 1})$
$k_{r} (M^{- 1} s^{- 1})$
1400
0.29
$1.1 \times 10^{- 6}$
1500
1.3
$1.4 \times 10^{- 5}$

Is the reaction endothermic or exothermic?