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Byju's Answer

Standard XII

Chemistry

Reaction Quotient

For the react...

Question

For the reaction $2 N_{2} O_{5} \to 4 N O_{2} + O_{2}$ , if the initial concentration of $N_{2} O_{5}$ is $7.2 m o l L^{- 1}$ and after $20$ minutes, $[N O_{2}]$ becomes $2.4 m o l L^{- 1}$ , then what will be rate of decomposition of $N_{2} O_{5}$ in $m o l L^{- 1} m i n^{- 1}$ ?

0.06

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Solution

The correct option is A $0.06$
$2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}$
$7.2 - 2 α$ $4 α$ $α$
Given $4 α = 2.4$
$\Rightarrow α = 0.6$
Change in $N_{2} O_{5}$ concentration= $Δ [N_{2} O_{5}] = 7.2 - (7.2 - 2 α)$
$\Rightarrow 2 α = 1.2 m o l L^{- 1}$
$∴$ Rate of decomposition of $N_{2} O_{5} = \frac{Δ [N_{2} O_{5}]}{Δ t} = \frac{1.2}{20} = 0.06 m o l L^{- 1} m i n^{- 1}$

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Similar questions

Q. For a reaction

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

;
Initial concentration of

N_{2} O_{5}

7.2

mol

L^{- 1}

and after

20

minutes

[N O_{2}] = 2.4

mol

L^{- 1}

, then what will be rate of decomposition of

N_{2} O_{5}

in mol

L^{- 1}

m i n^{- 1}

N_{2} O_{5}

dissociates as:

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

If concentration of 4 mol

L^{- 1}

reduces to 2.5 mol

L^{- 1}

in 3 minutes, what is the rate of production of

N O_{2}

Q. The decomposition of

N_{2} O_{5}

dissolved in carbontetrachloride occurs as follows.

N_{2} O_{5_{(S o l u t i o n)}} ⇌ 2 N O_{2_{(S o l u t i o n)}} + \frac{1}{2} O_{2 (g)}

.
This reaction is of first order and its rate constant is

5.0 \times 10^{- 4} s e c^{- 1}

. If initial concentration of

N_{2} O_{5}

for this reaction is

0.50 m o l e l i t r e^{- 1}

, then
a) What will be the initial reaction rate?
b) What will be half life period of this reaction?
c) What will be the concentrations of

N_{2} O_{5}

and

N O_{2}

at the end of

50

minutes after the starting of reaction?

Q. The decomposition of

N_{2} O_{5}

takes place according to I order as

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

Calculate:
(a) The rate constant, if instantaneous rate is

1.4 \times 10^{- 6} m o l l i t r e^{- 1} {sec}^{- 1}

when concentration of

N_{2} O_{5}

0.04 M

.
(b) The rate of reaction when concentration of

N_{2} O_{5}

1.20 M

.
(c) The concentration of

N_{2} O_{5}

when the rate of reaction will be

2.45 \times 10^{- 5} m o l l i t r e^{- 1} {sec}^{- 1}

Q. If the rate of decomposition of

N_{2} O_{5}

during a certain time internal is

2.4 \times 10^{- 4} m o l L^{- 1} m i n^{- 1}

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

What is the rate of formation of

N O_{2}

and

O_{2} m o l L^{- 1} m i n^{- 1}

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For the reaction 2N2O5→4NO2+O2, if the initial concentration of N2O5 is 7.2molL−1 and after 20 minutes, [NO2] becomes 2.4 molL−1, then what will be rate of decomposition of N2O5 in molL−1min−1 ?

The correct option is A 0.06 2N2O5⟶4NO2+O27.2−2α 4α αGiven 4α=2.4⇒α=0.6Change in N2O5 concentration= Δ[N2O5]=7.2−(7.2−2α) ⇒2α=1.2molL−1∴ Rate of decomposition of N2O5=Δ[N2O5]Δt=1.220=0.06molL−1min−1

For the reaction $2 N_{2} O_{5} \to 4 N O_{2} + O_{2}$ , if the initial concentration of $N_{2} O_{5}$ is $7.2 m o l L^{- 1}$ and after $20$ minutes, $[N O_{2}]$ becomes $2.4 m o l L^{- 1}$ , then what will be rate of decomposition of $N_{2} O_{5}$ in $m o l L^{- 1} m i n^{- 1}$ ?