Observe the following reactions at T ( K ). I. A \rightarrow products. II. 5 Br ^{-}( aq )+ BrO _3{ }^{-}( aq )+6 H ^{+}( aq ) \rightarrow 3 Br _2( aq )+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{∆ [ Br ^{-}] }{∆ 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 ? [23 jan 2026 Shift 2]

Chemical Kinetics Part 2

Section: Chemistry

Question : 7 of 111

Marks: +1, -0

Observe the following reactions at T(K).
I. A⟶ products.
II. 5Br−(aq)+BrO3‌−(aq)+6H+(aq)⟶3Br2(aq)+3H2O(l)
Both the reactions are started at 10.00 am .
The rates of these reactions at 10.10 am are same. The value of −‌

∆[Br−]

∆t

at 10.10 am is 2×10−4molL−1min−1. The concentration of A at 10.10 am is 10−2molL−1. What is the first order rate constant (in min−1 ) of reaction I ?

[23 jan 2026 Shift 2]

4×10−3
2×10−3
10−3
10−2

Validate

Go to Question:

Prev Question

Next Question