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(B) For a general reaction $aA + bB ightarrow cC + dD$,the rate of reaction is given by: $	ext{Rate} = -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b}

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$2x + y \rightarrow 2z$

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(B) For a general reaction $aA + bB ightarrow cC + dD$,the rate of reaction is given by: $	ext{Rate} = -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$.Comparing this with the given expression $-\frac{1}{2} \frac{d[x]}{dt} = -\frac{d[y]}{dt} = \frac{1}{2} \frac{d[z]}{dt}$,we can identify the stoichiometric coefficients:For reactant $x$,the coefficient is $2$.For reactant $y$,the coefficient is $1$.For product $z$,the coefficient is $2$.Thus,the balanced chemical equation is $2x + y ightarrow 2z$.

If the instantaneous rate of reaction is stated as $-\frac{1}{2} \frac{d[x]}{dt} = -\frac{d[y]}{dt} = \frac{1}{2} \frac{d[z]}{dt}$,identify the reaction.

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