For the reaction A + 2B to C + D,if -frac{d[A | vedclass

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(A) The rate of reaction for $A + 2B 	o C + D$ 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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$1.0 	imes 10^{-3} \ mol \ L^{-1} s^{-1}$

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

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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