The three experimental data for determine the differential rate of reaction $Cl _{2( g )} + 2NO _{( g )} \rightarrow 2 NOCl_{( g )}$ at $310\, K$ temperature.
$(a)$ Derive differential rate of reaction.
$(b)$ Calculate order of reaction.
$(c)$ Calculate value of rate constant.
The three experimental data for determine the differential rate of reaction $Cl _{2( g )} + 2NO _{( g )} \rightarrow 2 NOCl_{( g )}$ at $310\, K$ temperature.
$(a)$ Derive differential rate of reaction.
$(b)$ Calculate order of reaction.
$(c)$ Calculate value of rate constant.
$(a)$ $-\frac{d\left[\mathrm{Cl}_{2}\right]}{d t}=-\frac{d[\mathrm{NO}]}{d t}=k[\mathrm{NO}]^{2}\left[\mathrm{Cl}_{2}\right]^{1}$
$(b)$ Order of reaction $=2+1=3$
$(c)$ $175 \mathrm{~L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}$ ]
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Rate $mol\,L^{-1}\,s^{-1}$
$[A]$ $mol\,L^{-1}$
$[B]$ $mol\,L^{-1}$
$0.10$
$20$
$0.5$
$0.40$
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$0.5$
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| $0.10$ | $20$ | $0.5$ |
| $0.40$ | $x$ | $0.5$ |
| $0.80$ | $40$ | $y$ |
What is the value of $x$ and $y ?$
- [JEE MAIN 2023]
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For the reaction, $2A + B\,\to $ products , when the concentrations of $A$ and $B$ both were doubled, the rate of the reaction increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $2.4 \,mol\,L^{-1}\,s^{-1}.$ When the concentration of $A$ alone is doubled, the rate increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $0.6\,mol\,L^{-1}\,s^{-1}.$ Which one of the following statements is correct?
- [JEE MAIN 2019]