The equilibrium constant forr the reaction- N 2 g - O 2 g - 2 NO g at temperature T is 4 - 10-4- The value of K C for the reaction NO g -1-2 N 2 g -1-2 O 2 g at the same temperature is-A- 2-5 - 102B- 4 - 10-4C- 0-02D- 50

The correct option is D 50N_2(g) + O_2 (g) ⇋ 2NO(g) K_c = [NO]^2[NO_2][O_2] = 4 × 10^ 4 NO(g) ⇋12 N_2 (g) + 12O_2 (g) K_c^` = [n_2]^12[o_2]^12[NO] = 1√(K_c ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Gibb's Energy and Nernst Equation

The equilibri...

Question

The equilibrium constant forr 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 $N O (g) ⇋ \frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g)$ at the same temperature is:

2.5 \times 10^{2}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

0.02

No worries! We‘ve got your back. Try BYJU‘S free classes today!

4 \times 10^{- 4}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

50

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $50$
$N_{2} (g) + O_{2} (g) ⇋ 2 N O (g) K_{c} = \frac{[N O]^{2}}{[N O_{2}] [O_{2}]} = 4 \times 10^{- 4} N O (g) ⇋ \frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) K_{c}^{‘} = \frac{[n_{2}]^{\frac{1}{2}} [o_{2}]^{\frac{1}{2}}}{[N O]} = \frac{1}{\sqrt{K_{c}}} = \frac{1}{\sqrt{4 \times 10^{- 4}}} = \frac{1}{2 \times 10^{- 2}} = \frac{100}{2} = 50$

Suggest Corrections

Similar questions

Q. The equilibrium constant

(K_{c})

for the reaction,

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

at room temperature

T

4 \times 10^{- 4}

. The value of

K_{c}

for

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

at the same

T

is:

Q. The equilibrium constant for the reaction,

N_{2} (g) + O_{2} (g) ⇋ 2 N O (g)

at temperature

T

4 \times 10^{- 4}

The value of

K_{c}

for the reaction

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

at the same temperature is:

Q. The equilibrium constant for the reaction

N_{2} (g) + O_{2} (g) = 2 N O (g)

at temperature

T

4 \times 10^{- 4}

. The value of

K_{c}

for the reaction:

N O (g)

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

at the same temperature is :

Q. The equilibrium constant (

K_{c}

) for the reaction

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

at temperature

T

4 \times 10^{- 4}

. The value of

K_{P}

for the reaction

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

at the same temperature is:

Q. The equilibrium constant

(K_{c})

for the reaction

N_{2} (g) + O_{2} (g) \to 2

(g)

at temperature

T

4 \times 10^{- 4}

. The value of

K_{c}

for the reaction,

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

at the same temperature is:

Join BYJU'S Learning Program

The equilibrium constant forr the reaction, N2(g)+O2(g)⇋2NO(g) at temperature T is 4×10−4. The value of Kc for the reaction NO(g)⇋12N2(g)+12O2(g) at the same temperature is:

The correct option is D 50N2(g)+O2(g)⇋2NO(g)Kc=[NO]2[NO2][O2]=4×10−4NO(g)⇋12N2(g)+12O2(g)K‘c=[n2]12[o2]12[NO]=1√Kc=1√4×10−4=12×10−2=1002=50

The equilibrium constant forr 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 $N O (g) ⇋ \frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g)$ at the same temperature is: