The reaction that occurs in a breath analyser | vedclass

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Question

(C) From the stoichiometry of the reaction: $2 K_{2}Cr_{2}O_{7} + 8 H_{2}SO_{4} + 3 C_{2}H_{6}O$ $\rightarrow 2 Cr_{2}(SO_{4})_{3} + 3 C_{2}H_{4}O_{2}

Vedclass · Accepted Answer

$4$

Vedclass · Answer

(C) From the stoichiometry of the reaction: $2 K_{2}Cr_{2}O_{7} + 8 H_{2}SO_{4} + 3 C_{2}H_{6}O$ $ightarrow 2 Cr_{2}(SO_{4})_{3} + 3 C_{2}H_{4}O_{2} + 2 K_{2}SO_{4} + 11 H_{2}O$.The rate of reaction is given by: $	ext{Rate} = -\frac{1}{3} \frac{d[C_{2}H_{6}O]}{dt} = \frac{1}{2} \frac{d[Cr_{2}(SO_{4})_{3}]}{dt}$.Given,$\frac{d[Cr_{2}(SO_{4})_{3}]}{dt} = 2.67 \ mol \ min^{-1}$.Therefore,$-\frac{d[C_{2}H_{6}O]}{dt} = \frac{3}{2} 	imes \frac{d[Cr_{2}(SO_{4})_{3}]}{dt}$.$-\frac{d[C_{2}H_{6}O]}{dt} = \frac{3}{2} 	imes 2.67 = 4.005 \ mol \ min^{-1}$.The nearest integer is $4$.

Similar Questions

Find the rate of the following reaction: $2 \ N_2O_{5(g)} \rightarrow 4 \ NO_{2(g)} + O_{2(g)}$ if the concentration of $NO_2$ increases to $5.2 \times 10^{-3} \ M$ in $100 \ s$.

Select the correct reaction for the given rate: $\text{rate} = -\frac{1}{6} \frac{d[A]}{dt} = -\frac{1}{4} \frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} = \frac{1}{4} \frac{d[D]}{dt}$

Which one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?

The rate of reaction is expressed as
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is:

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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