For a reaction 2N2O5g- 4NO2g- O2g - the rate and rate constant are 1-02- 10-4 mol L-1 s-1 and 3-4-10-5 s-1 respectively- The concentration of N2O5 at this time will be-

The correct option is C 3 mol/LThe given reaction is 2N_2O_5→ 4NO_2 + O_2 Given, rate=R = 1.02×10^ 4 mol L^ 1s^ 1 Rate constant = nbsp;k = 3.010 s^ 1 Reactio ...

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Standard XII

Chemistry

Factors Affecting Rate of Reaction

For a reactio...

Question

For a reaction $2 N_{2} O_{5} (g)$ $\to 4 N O_{2} (g) + O_{2} (g)$ , the rate and rate constant are $1.02 \times 10^{- 4}$ $m o l L^{- 1} s^{- 1}$ and $3.4 \times 10^{- 5} s^{- 1}$ respectively. The concentration of $N_{2} O_{5}$ at this time will be:

1.732 mol/L

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3 mol/L

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1.02 \times 10^{- 4}

mol/L

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3.2 \times 10^{5}

mol/L

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Solution

The correct option is B 3 mol/L
The given reaction is
$2 N_{2} O_{5} \to 4 N O_{2} + O_{2}$
Given, rate= $R = 1.02 \times 10^{- 4} m o l L^{- 1} s^{- 1}$
Rate constant = $k = 3.010 s^{- 1}$
Reaction follows $1^{s t}$ order kinetics as unit of k is $s^{- 1}$
Rate = $k [N_{2} O_{5}]$
$1.02 \times 10^{- 4}$ = $(3.4 \times 10^{- 5})$ $[N_{2} O_{5}]$
$[N_{2} O_{5}]$ =3 mol/L

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Similar questions

Q. For a reaction

2 N_{2} O_{5} (g)

\to 4 N O_{2} (g) + O_{2} (g)

, the rate and rate constant are

1.02 \times 10^{- 4}

m o l L^{- 1} s^{- 1}

and

3.4 \times 10^{- 5} s^{- 1}

respectively. The concentration of

N_{2} O_{5}

at this time will be:

Q. For the reaction,

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

rate and rate constant are

1.02 \times 10^{- 4} m o l L^{- 1} s^{- 1}

and

3.4 \times 10^{- 5} s^{- 1}

respectively. The concentration of

N_{2} O_{5}

in mol

L^{- 1}

will be:

Q. How long does it take for reactant concentration to decrease from

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

2 \times 10^{- 4} m o l L^{- 1}

in a zero order reaction.

Rate constant of the reaction, k = 5 \times 10^{- 8} m o l L^{- 1} s^{- 1}

Q. For the reaction,

2 N_{2} O_{5} ⇌ 4 N O_{2} + O_{2}

rate and rate constant are

2.40 \times 10^{- 5}

mol

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

and

3 \times 10^{- 5} s^{- 1}

respectively, then calculate the concentration of

N_{2} O_{5}

Q. Rate For the reaction

A + B \to p r o d u c t s

, what will be the order of reaction with respect of

A

and

B

Exp.	$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	Initial rate $(m o l L^{- 1} s^{- 1})$
$1.$	$2.5 \times 10^{- 4}$	$3 \times 10^{- 5}$	$5 \times 10^{- 4}$
$2.$	$5 \times 10^{- 4}$	$6 \times 10^{- 5}$	$4 \times 10^{- 3}$
$3.$	$1 \times 10^{- 3}$	$6 \times 10^{- 5}$	$1.6 \times 10^{- 2}$

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For a reaction 2N2O5(g)→4NO2(g)+O2(g) , the rate and rate constant are 1.02×10−4 mol L−1 s−1 and 3.4×10−5 s−1 respectively. The concentration of N2O5 at this time will be:

The correct option is B 3 mol/LThe given reaction is 2N2O5→4NO2+O2 Given, rate=R=1.02×10−4 mol L−1s−1 Rate constant = k=3.010 s−1 Reaction follows 1storder kinetics as unit of k is s−1 Rate = k[N2O5] 1.02×10−4 = (3.4×10−5)[N2O5] [N2O5]=3 mol/L

For a reaction $2 N_{2} O_{5} (g)$ $\to 4 N O_{2} (g) + O_{2} (g)$ , the rate and rate constant are $1.02 \times 10^{- 4}$ $m o l L^{- 1} s^{- 1}$ and $3.4 \times 10^{- 5} s^{- 1}$ respectively. The concentration of $N_{2} O_{5}$ at this time will be: