Give the definition of the following terms:
$(i)$ Rate of Reaction
$(ii)$ Average rate of reaction
$(iii)$ Instantaneous rate
$(i)$ Rate of Reaction
$(ii)$ Average rate of reaction
$(iii)$ Instantaneous rate
(N/A) $(i)$ Rate of Reaction: The change in concentration of any one of the reactants or products per unit time is called the rate of reaction.
$(ii)$ Average rate of reaction: The rate of reaction measured over a definite time interval $( \Delta t )$ is called the average rate of reaction. It is given by $r_{av} = -\frac{\Delta [R]}{\Delta t} = +\frac{\Delta [P]}{\Delta t}$.
$(iii)$ Instantaneous rate: The rate of reaction at a particular instant of time is called the instantaneous rate. It is determined by calculating the slope of the tangent to the concentration-time graph at that specific time $t$,given by $r_{inst} = -\frac{d[R]}{dt} = +\frac{d[P]}{dt}$ as $\Delta t \to 0$.
$(ii)$ Average rate of reaction: The rate of reaction measured over a definite time interval $( \Delta t )$ is called the average rate of reaction. It is given by $r_{av} = -\frac{\Delta [R]}{\Delta t} = +\frac{\Delta [P]}{\Delta t}$.
$(iii)$ Instantaneous rate: The rate of reaction at a particular instant of time is called the instantaneous rate. It is determined by calculating the slope of the tangent to the concentration-time graph at that specific time $t$,given by $r_{inst} = -\frac{d[R]}{dt} = +\frac{d[P]}{dt}$ as $\Delta t \to 0$.
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Similar Questions
Which of the following is a correct representation of the reaction rate for the reaction stated below?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
Find the average rate of formation of $NO_{2_{(g)}}$ in the following reaction:
$2 N_2O_{5_{(g)}} \rightarrow 4 NO_{2_{(g)}} + O_{2_{(g)}}$
Given that $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$
$2 N_2O_{5_{(g)}} \rightarrow 4 NO_{2_{(g)}} + O_{2_{(g)}}$
Given that $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$
For the decomposition of $A$ as shown below,calculate the rate of appearance of $B$ if the initial concentration of $A$ is $2 \ M$.
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$
Medium
View SolutionFor the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the reaction occurs under specific temperature and partial pressure conditions. The rate of formation of $NH_3$ is $0.001 \, kg \, h^{-1}$. The rate of consumption of $H_2$ under the same conditions is ...... $kg \, h^{-1}$.
Medium
View SolutionIf the instantaneous rate of reaction is given as $-\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$,then the reaction is represented as:
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