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Standard XII

Chemistry

Elementary and Complex Reactions

The decomposi...

Question

The decomposition of $N_{2} O_{5}$ in C $C l_{4}$ at 318K has been studied by monitoring the concentration of $N_{2} O_{5}$ in the solution. Initially the concentration of N2O5 is 2.33 mol L–1 and after 184 minutes, it is reduced to 2.08 mol L–1. The reaction takes place according to the equation 2 N2O5 (g) → 4 NO2 (g) + O2 (g) Calculate the average rate of this reaction in terms of hours, minutes and seconds. What is the rate of production of NO2 during this period?

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Solution

Average Rate 1 1 1 mol L N O2 5 2.08 2.33 2 2 t 184 min = 6.79 × 10–4 mol L–1/min = (6.79 × 10–4 mol L–1 min–1) × (60 min/1h) = 4.07 × 10–2 mol L–1/h = 6.79 × 10–4 mol L–1 × 1min/60s = 1.13 × 10–5 mol L–1s–1 It may be remembered that 1 NO2 Rate 4 t NO2 t 6.79 × 10–4 × 4 mol L–1 min–1 = 2.72 × 10–3 mol L–1min–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}

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. For the reaction

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

, if the initial concentration of

N_{2} O_{5}

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}

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

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. The decomposition of

N_{2} O_{5}

at 318 K according to the following equation follows first order reaction:

N_{2} O_{5} (g) \to 2 N O_{2} (g) + 1 / 2 O_{2} (g)

The initial concentration of

N_{2} O_{5}

was

1.24 \times 10^{- 2}

mol

L^{- 1}

and after 60 minutes was

0.20 \times 10^{- 2}

L^{- 1}

, Calculate the rate constant of the reaction at 318 K.

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