The rate of a reaction at 10 sec intervals are as follows-Time sec Rate mol L -1 sec -1 0 4-8- 10 -2 10 4-79- 10 -2 20 4-78- 10 -2 30 4-81- 10 -2What will be the order of the reaction-

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Zero Order Reaction

The rate of a...

Question

The rate of a reaction at $10$ sec intervals are as follows:
Time $(s e c)$ Rate
$(m o l L^{- 1} {s e c}^{- 1})$
$0$ $4.8 \times 10^{- 2}$
$10$ $4.79 \times 10^{- 2}$
$20$ $4.78 \times 10^{- 2}$
$30$ $4.81 \times 10^{- 2}$
What will be the order of the reaction?

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

A

B

\begin{matrix} T i m e (s e c o n d) & 0 & 10 & 20 R a t e (m o l L^{- 1} s^{- 1}) & 1.8 \times 10^{- 2} & 1.82 \times 10^{- 2} & 1.79 \times 10^{- 2} \end{matrix}

2 A + B \to C

2.57 \times 10^{- 5}

l i t r e

{m o l e}^{- 1}

{s e c}^{- 1}

10

2.65 \times 10^{- 5}

l i t r e

{m o l e}^{- 1}

{s e c}^{- 1}

20

2.55 \times 10^{- 5} l i t r e .

{m o l e}^{- 1}

{s e c}^{- 1}

30

2 A + B ⟶ C

2.57 \times 10^{- 5}

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

2.65 \times 10^{- 5}

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

2.55 \times 10^{- 5}

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

2 A + B \to C

2.57 \times 10^{- 5}

l t . m o l^{- 1}

s e c^{- 1}

2.65 \times 10^{- 5}

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

2.55 \times 10^{- 5}

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

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