Chemistry - Chemical Kinetics Question with Solution | TestHub

For a general reaction $aA+bB\to cC$, the rate of reaction is given by:

$\text{Rate}=-\frac{1}{a}\frac{\mathrm{d}[A]}{\mathrm{dt}}=-\frac{1}{b}\frac{\mathrm{d}[B]}{\mathrm{dt}}=\frac{1}{c}\frac{\mathrm{d}[C]}{\mathrm{dt}}$

The given rate expression is:

$-\frac{1}{2}\frac{\mathrm{d}[x]}{\mathrm{dt}}=-\frac{\mathrm{d}[y]}{\mathrm{dt}}=\frac{1}{2}\frac{\mathrm{d}[z]}{\mathrm{dt}}$

The negative signs indicate that $x$ and $y$ are reactants, while the positive sign indicates that $z$ is a product.

Comparing the given expression with the general rate equation, the stoichiometric coefficients are $2$ for $x$, $1$ for $y$, and $2$ for $z$.

Therefore, the balanced chemical equation is $2x+y\to 2z$.

Answer: $2x+y\to 2z$