If rate of consumption of O2 is 3-2 - 10-2 g L-1 min-1 in the formation of NO2 from N2 and O2- for the given reaction -2O2 - N2 - 2NO2- then the rate of reaction is- - - - -2O2 - N2 - 2NO2- - - N2 - O2 - NO2 - - - O2 - - - - - 3-2 - 10-2 g L-1 min-1 - - - - - -

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Standard VII

Chemistry

Effects of Hardness

If rate of co...

Question

If rate of consumption of O₂ is 3.2 × 10^–2 g L^–1 min^–1 in the formation of NO₂ from N₂ and O₂, for the given reaction [2O₂ + N₂ → 2NO₂], then the rate of reaction is

यदि दी गयी अभिक्रिया [2O₂ + N₂ → 2NO₂] के लिए N₂ तथा O₂ से NO₂ के निर्माण में O₂ के प्रयुक्त होने की दर 3.2 × 10^–2 g L^–1 min^–1 है, तो अभिक्रिया का वेग है

1.6 × 10^–2 mol L^–1 min^–1

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5 × 10^–4 mol L^–1 min^–1

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1 × 10^–3 mol L^–1 min^–1

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2 × 10^–4 mol L^–1 min^–1

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The correct option is B 5 × 10^–4 mol L^–1 min^–1
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Similar questions

Q. In a reaction,

N_{2} O_{5} \to 2 N O_{2} + \frac{1}{2} O_{2}

, the rate of disappearance of

N_{2} O_{5}

6.5 \times 10^{- 3}

m o l

L^{- 1} s^{- 1}

. Compute the rates of formation of

N O_{2}

and

O_{2}

Q. For the reaction;

N_{2} O_{5} ⟶ 2 {N O}_{2} + \frac{1}{2} O_{2}

,
given:

- \frac{d [N_{2} O_{5}]}{d t} = K_{1} [N_{2} O_{5}]

- \frac{d [{N O}_{2}]}{d t} = K_{2} [{N O}_{2}]

,
and

- \frac{d [O_{2}]}{d t} = K_{3} [O_{2}]

The relation between

K_{1}, K_{2}, K_{3}

is:

Q. The equilibrium constant for the reaction,

N_{2} + 2 O_{2} ⇌ 2 N O_{2}

100

. The equilibrium constant for the reactions:
(a)

2 N O_{2} ⇌ N_{2} + 2 O_{2}

K_{1}

(b)

N O_{2} ⇌ \frac{1}{2} N_{2} + O_{2}

K_{2}

Find the value of

K_{1} \times K_{2}

Q. For the reaction

2 {N O}_{2} ⟶ N_{2} O_{2} + O_{2}

, rate expression is as follows;

- \frac{d [{N O}_{2}]}{d t} = k {[{N O}_{2}]}^{n}

, where

k = 3 \times 10^{- 3} {m o l}^{- 1} L {s e c}^{- 1}

. If the rate of formation of oxygen is

1.5 \times 10^{- 4} m o l L^{- 1} {s e c}^{- 1}

, then the molar concentration of

{N O}_{2}

in mole

L^{- 1}

is:

Q. Decomposition of

N_{2} O_{5}

is expressed by the equation,

N_{2} O_{5} ⟶ 2 N O_{2} + \frac{1}{2} O_{2}

.
If during a certain time interval, the rate of decomposition of

N_{2} O_{5}

1.8 \times 10^{- 3}

m o l

{l i t r e}^{- 1}

{m i n}^{- 1}

, what will be the rates of formation of

N O_{2}

and

O_{2}

during the same interval?

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The correct option is B 5 × 10–4 mol L–1 min–1Solution

The correct option is B 5 × 10^–4 mol L^–1 min^–1
Solution