The instantaneous rate of disappearance of Mn | vedclass

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(B) Given: The rate of disappearance of $MnO_4^-$ is $-\frac{d[MnO_4^-]}{dt} = 4.56 	imes 10^{-3} \ M s^{-1}$.From the stoichiometry of the reaction

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$1.14$

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(B) Given: The rate of disappearance of $MnO_4^-$ is $-\frac{d[MnO_4^-]}{dt} = 4.56 	imes 10^{-3} \ M s^{-1}$.From the stoichiometry of the reaction $2MnO_4^- + 10I^{-} + 16H^{+} 	o 2Mn^{2+} + 5I_2 + 8H_2O$,the rate expression is:$-\frac{1}{2} \frac{d[MnO_4^-]}{dt} = \frac{1}{5} \frac{d[I_2]}{dt}$.Rearranging to find the rate of appearance of $I_2$:$\frac{d[I_2]}{dt} = -\frac{5}{2} \frac{d[MnO_4^-]}{dt}$.Substituting the given value:$\frac{d[I_2]}{dt} = \frac{5}{2} 	imes (4.56 	imes 10^{-3}) \ M s^{-1} = 2.5 	imes 4.56 	imes 10^{-3} \ M s^{-1} = 11.4 	imes 10^{-3} \ M s^{-1} = 1.14 	imes 10^{-2} \ M s^{-1}$.

$t/s$	$0$	$50$	$100$	$150$	$200$	$300$	$400$	$700$	$800$
$[C_{4}H_{9}Cl]/mol\ L^{-1}$	$0.100$	$0.0905$	$0.0820$	$0.0741$	$0.0671$	$0.0549$	$0.0439$	$0.0210$	$0.017$

The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ M s^{-1}$.
$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$
The rate of appearance of $I_2$ is $...... \times 10^{-2} \ M s^{-1}$.

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The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ M s^{-1}$.$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$The rate of appearance of $I_2$ is $...... \times 10^{-2} \ M s^{-1}$.