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MCQEasyJEE Main 2026 · 23 January, Shift 2Rate of Reaction

Chemistry Question from JEE Main 2026 · 23 January, Shift 2

Observe the following reactions at T(K)T(\text{K}). I. A→productsA \to \text{products}. II. 5Br−+BrO3−+6H+→3Br2+3H2O5Br^- + BrO_3^- + 6H^+ \to 3Br_2 + 3H_2O. Both the reactions are started at 10.00 am10.00 \, \text{am}. The rates of these reactions at 10.10 am10.10 \, \text{am} are same. The value of −d[Br−]dt-\frac{d[Br^-]}{dt} at 10.10 am10.10 \, \text{am} is 2×10−4 mol L−1 min−12 \times 10^{-4} \, \text{mol L}^{-1} \, \text{min}^{-1}. The concentration of AA at 10.10 am10.10 \, \text{am} is 10−2 mol L−110^{-2} \, \text{mol L}^{-1}. What is the first order rate constant (in min−1\text{min}^{-1}) of reaction I?

  • A

    2×10−32 \times 10^{-3}

  • B

    4×10−34 \times 10^{-3}

  • C

    10−210^{-2}

  • D

    10−310^{-3}

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