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Rate of Reaction

For the react...

Question

For the reaction,
$A + B \to C$
The concentration of $A$ initially was observed to be $0.2 m o l / L$ and the concentration of $A$ after $20 m i n$ was found out to be $0.16 m o l / L$ .

Calculate the average rate of reaction $(r_{a v})$ for first $20 m i n$ in $m o l L^{- 1} m i n^{- 1}$

1 \times 10^{- 3}

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5 \times 10^{- 4}

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1 \times 10^{- 4}

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2 \times 10^{- 3}

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Solution

The correct option is D $2 \times 10^{- 3}$
Average rate of reaction:
$r_{a v} = - \frac{[A]_{f i n a l} - [A]_{i n i t i a l}}{t_{f i n a l} - t_{i n i t i a l}} = - \frac{Δ A}{Δ t}$
Here $[A]_{f i n a l}, [A]_{i n i t i a l} are the concentration of reactant A at t_{f i n a l}, t_{i n i t i a l} respectively$
$r_{a v} = - \frac{0.16 - 0.2}{20} m o l L^{- 1} m i n^{- 1}$
$r_{a v} = 2 \times 10^{- 3} m o l L^{- 1} m i n^{- 1}$

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Rate of Reaction

Standard VII Chemistry

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For the reaction, A+B→C The concentration of A initially was observed to be 0.2 mol/L and the concentration of A after 20 min was found out to be 0.16 mol/L. Calculate the average rate of reaction (rav) for first 20 min in mol L−1min−1

The correct option is D 2×10−3Average rate of reaction: rav=−[A]final−[A]initialtfinal−tinitial=−ΔAΔt Here [A]final,[A]initial are the concentration of reactant A at tfinal,tinitial respectively rav=−0.16−0.220 mol L−1min−1 rav=2×10−3 mol L−1min−1

For the reaction,
$A + B \to C$
The concentration of $A$ initially was observed to be $0.2 m o l / L$ and the concentration of $A$ after $20 m i n$ was found out to be $0.16 m o l / L$ .

Calculate the average rate of reaction $(r_{a v})$ for first $20 m i n$ in $m o l L^{- 1} m i n^{- 1}$