(B) The rate of a chemical reaction is defined as the change in concentration of any of the reactants or products per unit time. Mathematically,for a

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rate of consumption of reactant and formation of product.

(B) The rate of a chemical reaction is defined as the change in concentration of any of the reactants or products per unit time. Mathematically,for a reaction $A \rightarrow B$,the rate can be expressed as: Rate $= -\frac{d[A]}{dt} = \frac{d[B]}{dt}$. Thus,it is expressed in terms of both the rate of consumption of reactants and the rate of formation of products.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

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The rate of a chemical reaction can be expressed in terms of:

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A
rate of consumption of reactant only.
B
rate of consumption of reactant and formation of product.
C
rate of formation of products only.
D
rate of consumption of catalyst.

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Chemical Kinetics

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Rate of a reaction

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For the chemical reaction $A + 2B \to 3C$,which of the following expressions correctly represents the rate of reaction?

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What is the rate of reaction?

Medium

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Thermal decomposition of $N_2O_5$ occurs as per the equation below:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is:

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Write the following equations for the reaction $R \to P$: $(i)$ Average rate $(ii)$ Instantaneous rate.

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In the following reaction: $xA \to yB$,$\log \left[ -\frac{d[A]}{dt} \right] = \log \left[ \frac{d[B]}{dt} \right] + \log 2$,where the negative sign indicates the rate of disappearance of the reactant. Thus,$x : y$ is:

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The rate of a chemical reaction can be expressed in terms of:

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For the chemical reaction $A + 2B \to 3C$,which of the following expressions correctly represents the rate of reaction?

What is the rate of reaction?

Thermal decomposition of $N_2O_5$ occurs as per the equation below:$2N_2O_5 \longrightarrow 4NO_2 + O_2$The correct statement is:

Write the following equations for the reaction $R \to P$: $(i)$ Average rate $(ii)$ Instantaneous rate.

In the following reaction: $xA \to yB$,$\log \left[ -\frac{d[A]}{dt} \right] = \log \left[ \frac{d[B]}{dt} \right] + \log 2$,where the negative sign indicates the rate of disappearance of the reactant. Thus,$x : y$ is:

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Thermal decomposition of $N_2O_5$ occurs as per the equation below:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is: