For $n^{th}$ order reaction where $(n < 1)$
For $n^{th}$ order reaction where $(n < 1)$
- A
${t_{100\% }} = \frac{1}{{n-1}}\,\frac{{A_0^{n - 1}}}{K}$
- B
${t_{100\% }} = \frac{1}{{1-n}}\,\frac{{\left[ A \right]_0^{1 - n}}}{K}$
- C
${t_{100\% }} = \frac{1}{n}\,\frac{{\left[ A \right]_0^{n - 1}}}{K}$
- D
${t_{100\% }} = \frac{1}{{1 - n}}\,\frac{{A_0^n}}{K}$
Similar Questions
The decomposition of $NH _{3}$ on $Pt$ surface is a zero order reaction. If the value of rate constant is $2 \times 10^{-4}\,mole $ $liter^{-1}\, sec ^{-1}$ The rate of appearance of $N _{2}$ and $H _{2}$ are respectively.
The decomposition of $NH _{3}$ on $Pt$ surface is a zero order reaction. If the value of rate constant is $2 \times 10^{-4}\,mole $ $liter^{-1}\, sec ^{-1}$ The rate of appearance of $N _{2}$ and $H _{2}$ are respectively.
- [AIIMS 2019]
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
For a chemical reaction, $A + 2B \to C + D$, the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\, times$, then rate of reaction also increases $2\, times$. The order of this reaction is
For a chemical reaction, $A + 2B \to C + D$, the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\, times$, then rate of reaction also increases $2\, times$. The order of this reaction is
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(ii)$ $H _{2} O _{2}( aq )+3 I ^{-}( aq )+2 H ^{+} \rightarrow 2 H _{2} O ( l )+ I _{3}^{-} \quad$ Rate $=k\left[ H _{2} O _{2}\right][ I ]$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(ii)$ $H _{2} O _{2}( aq )+3 I ^{-}( aq )+2 H ^{+} \rightarrow 2 H _{2} O ( l )+ I _{3}^{-} \quad$ Rate $=k\left[ H _{2} O _{2}\right][ I ]$
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?