For the reaction,XA + YB rightarrow ZC,if fra | vedclass

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(A) For a general reaction $XA + YB \rightarrow ZC$,the rate of reaction is given by:Rate $= -\frac{1}{X} \frac{d[A]}{dt} = -\frac{1}{Y} \frac{d[B]}{d

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The value of $X = Y = Z = 3$

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(A) For a general reaction $XA + YB ightarrow ZC$,the rate of reaction is given by:Rate $= -\frac{1}{X} \frac{d[A]}{dt} = -\frac{1}{Y} \frac{d[B]}{dt} = \frac{1}{Z} \frac{d[C]}{dt}$Given that $\frac{-d[A]}{dt} = \frac{-d[B]}{dt} = \frac{d[C]}{dt}$,we can equate these to the rate expression:$\frac{1}{X} (	ext{Rate}) = \frac{1}{Y} (	ext{Rate}) = \frac{1}{Z} (	ext{Rate})$This implies that $X = Y = Z$. Since the coefficients in a balanced chemical equation must be equal for the rates of disappearance and appearance to be equal,the simplest integer ratio is $X = Y = Z = 1$. However,looking at the options provided,the statement $X = Y = Z$ is implied by the equality of the rates. Given the options,the most consistent choice is that the coefficients are equal.

For the reaction,$XA + YB \rightarrow ZC$,if $\frac{- d [ A ]}{ dt } = \frac{- d [ B ]}{ dt } = \frac{d [ C ]}{ dt },$ then the correct statement among the following is:

Similar Questions

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of disappearance of $N_{2(g)}$ is $2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$. What is the rate of appearance of $NH_{3(g)}$?

Why does the rate of reaction increase with respect to product?

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