(A) The rate of reaction for $A + 2B \to C + D$ is given by the expression: Rate $= -\frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt} = \frac{d[C]}{dt}

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$1.0 \times 10^{-3} \ mol \ L^{-1} s^{-1}$

(A) The rate of reaction for $A + 2B \to C + D$ is given by the expression: Rate $= -\frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt} = \frac{d[C]}{dt} = \frac{d[D]}{dt}$ Given that $-\frac{d[A]}{dt} = 5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,we can equate this to the rate of disappearance of $B$: $-\frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt}$ $-\frac{d[B]}{dt} = 2 \times (-\frac{d[A]}{dt})$ $-\frac{d[B]}{dt} = 2 \times (5 \times 10^{-4} \ mol \ L^{-1} s^{-1}) = 1.0 \times 10^{-3} \ mol \ L^{-1} s^{-1}$

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

For the reaction $A + 2B \to C + D$,if $-\frac{d[A]}{dt} = 5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,then what is the value of $-\frac{d[B]}{dt}$?

A
$1.0 \times 10^{-3} \ mol \ L^{-1} s^{-1}$
B
$5.0 \times 10^{-4} \ mol \ L^{-1} s^{-1}$
C
$2.5 \times 10^{-3} \ mol \ L^{-1} s^{-1}$
D
$2.5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$

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Rate of a reaction

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For the reaction $A + 2B \to C + D$,if $-\frac{d[A]}{dt} = 5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,then what is the value of $-\frac{d[B]}{dt}$?

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For the reaction $2N_2O_{5(g)} \to 4NO_{2(g)} + O_{2(g)}$,if the concentration of $NO_2$ increases by $5.2 \times 10^{-3} \ M$ in $100 \ s$,then the rate of reaction will be:

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