Observe the following reactions at T(K). I. II. Both the reactions are started at 10.00 am. The rates of these reactions at 10.10 am are same. The valu

Question

Observe the following reactions at T(K).

I. $A \to p r o d u c t s$

II. $5 {Br}^{-} (a q) + {BrO}_{3}^{-} (a q) + 6 H^{+} (a q) \to 3 {Br}_{2} (a q) + 3 H_{2} O (l)$

Both the reactions are started at 10.00 am. The rates of these reactions at 10.10 am are same. The value of $- \frac{Δ [{Br}^{-}]}{Δ t}$ at 10.10 am is $2 \times 10^{- 4} mol L^{- 1} \min^{- 1}$ . The concentration of A at 10.10 am is $10^{- 2} mol L^{- 1}$ . What is the first order rate constant (in $\min^{- 1}$ ) of reaction $I$ ? [2026]

Smart Achievers · Accepted Answer

(2)

$A \to p r o d u c t s$

$Rate of reaction = - \frac{1}{5} \frac{Δ [{Br}^{-}]}{Δ t} = \frac{1}{5} \times (2 \times 10^{- 4}) = 4 \times 10^{- 5}$

$For reaction A \to P$

$at t = 10 minutes$

$Rate of reaction = 4 \times 10^{- 5} = k [A]$

$k = 4 \times 10^{- 3} {min}^{- 1}$

Solution

1 $10^{- 2}$

2 $4 \times 10^{- 3}$

3 $10^{- 3}$

4 $2 \times 10^{- 3}$

Ans.
(2)

$At t = 10 minutes$

$Rate of reaction = - \frac{1}{5} \frac{Δ [{Br}^{-}]}{Δ t} = \frac{1}{5} \times (2 \times 10^{- 4}) = 4 \times 10^{- 5}$

$For reaction A \to P$

$at t = 10 minutes$

$Rate of reaction = 4 \times 10^{- 5} = k [A]$

$k = 4 \times 10^{- 3} {min}^{- 1}$

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Solution

1 10-2

2 4×10-3

3 10-3

4 2×10-3