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Standard VII

Chemistry

First Order Reaction

For a reactio...

Question

For a reaction $A \to B, Δ C_{B}$ is 0.01 moles per litre in 20 seconds, what is the average rate of reaction?

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

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

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

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

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Solution

The correct option is A $5 \times 10^{- 4} m o l e L^{- 1} s e c^{- 1}$
It is given that for the reaction, $A \to B$ , change in concentration $(Δ C_{B})$ is $0.01$ moles per litre in $20$ seconds.
Rate of reaction $= \frac{0.01}{20} = 5 \times 10^{- 4} m o l {l i t}^{- 1} s^{- 1}$

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Similar questions

Q. The rate constant (K) for the reaction,

2 A + B \to

Product was found to be

2.5 \times 10^{- 5}

litre

m o l^{- 1} s e c^{- 1}

after 15 sec,

2.60 \times 10^{- 5} l i t r e m o l^{- 1} s e c^{- 1}

after 30 sec and

2.55 \times 10^{- 5} l i t r e m o l^{- 1} s e c^{- 1}

after 50 sec. The order of reaction is:

Q. The rate constant

(K)

for the reaction

2 A + B \to

product, was found to be

2.5 \times 10^{- 5}

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

after

15 s e c

2.60 \times 10^{- 5} l i t m o l^{- 1} s e c^{- 1}

after

30 s e c

and

2.55 \times 10^{- 5}

l i t m o l^{- 1} s e c^{- 1}

after

50 s e c

. The order of reaction is:

Q. The rate constant of the reaction :

2 A + B \to C

2.57 \times 10^{- 5}

l t . m o l^{- 1}

s e c^{- 1}

after 10 sec,

2.65 \times 10^{- 5}

l t . m o l^{- 1} s e c^{- 1}

after 20 sec and

2.55 \times 10^{- 5}

l t . m o l^{- 1} s e c^{- 1}

after 30 sec. The order of the reaction is :

Q. The rate constant for the reaction,

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

, is

3.0 \times 10^{- 5} s e c^{- 1}

. If the rate is

2.40 \times 10^{- 5}

mol

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

, then the concentration of

N_{2} O_{5}

( in mol

l i t r e^{- 1}

) is:

Q. In a reaction;

H_{2} + I_{2} \to 2 H I

, the rate of dissappearance of

I_{2}

is found to be

10^{- 6} m o l l i t r e^{- 1} s e c^{- 1}

. If the corresponding rate of appearance of HI is

x \times 10^{- 6} m o l l i t r e^{- 1} s e c^{- 1}

then

x

is:

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For a reaction A→B, ΔCB is 0.01 moles per litre in 20 seconds, what is the average rate of reaction?

The correct option is A 5×10−4mole L−1sec−1It is given that for the reaction, A→B, change in concentration (ΔCB) is 0.01 moles per litre in 20 seconds.Rate of reaction =0.0120=5×10−4 mol lit−1s−1

For a reaction $A \to B, Δ C_{B}$ is 0.01 moles per litre in 20 seconds, what is the average rate of reaction?

The correct option is A $5 \times 10^{- 4} m o l e L^{- 1} s e c^{- 1}$
It is given that for the reaction, $A \to B$ , change in concentration $(Δ C_{B})$ is $0.01$ moles per litre in $20$ seconds.
Rate of reaction $= \frac{0.01}{20} = 5 \times 10^{- 4} m o l {l i t}^{- 1} s^{- 1}$