320489
For the decomposition of a compound \(\mathrm{AB}\) at \(600 \mathrm{~K}\), the following data were obtained The order for the decomposition of AB is
1 0
2 1
3 2
4 1.5
Explanation:
Let rate equation be, \(\text { rate }=K[A B]^{\mathrm{n}}\) Case (1), \(2.75 \times 10^{-8}=\mathrm{k}[0.2]^{\mathrm{n}}\) Case (2), \(11 \times 10^{-8}=\mathrm{k}[0.40]^{\mathrm{n}}\) Case (3), \(24.75 \times 10^{-8}=\mathrm{k}[0.6]^{\mathrm{n}}\) Divided (2) by (1), \(\dfrac{11 \times 10^{-8}}{2.75 \times 10^{-8}}=\dfrac{[0.40]^{\mathrm{n}}}{[0.2]^{\mathrm{n}}} \Rightarrow 2^{\mathrm{n}}=4 \Rightarrow \mathrm{n}=2\) \(\therefore\) Order of reaction is 2 .
CHXII04:CHEMICAL KINETICS
320490
For a reaction \(\mathrm{A}+2 \mathrm{~B} \rightarrow\) Products, when concentration of \(\mathrm{B}\) alone is increased half life remains the same. If concentration of A alone is doubled, rate remains the same. The unit of rate constant of the reaction is
As \([' B ']\) increase, \(t_{\dfrac{1}{2}}\) remains same i.e. \(1^{\text {st }}\) order with respect to ' \(\mathrm{B}\) ' rate \(=\mathrm{k}[\mathrm{A}]^{0}[\mathrm{~B}]^{1}\) overall order \(=1\) \(\therefore\) units of \(\mathrm{k}=\mathrm{S}^{-1}\)
CHXII04:CHEMICAL KINETICS
320491
The half-lives of two samples are \(0.1 \mathrm{~s}\) and 0.8 s and their respective concentrations are \(400 \mathrm{~mol} \mathrm{~L}^{-1}\) and \(50 \mathrm{~mol} \mathrm{~L}^{-1}\). The order of the reaction is
320492
Using the data given below, the order and rate constant for the reaction: \(\mathrm{CH}_{3} \mathrm{CHO}(\mathrm{g}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{CO}(\mathrm{g})\) would be
320489
For the decomposition of a compound \(\mathrm{AB}\) at \(600 \mathrm{~K}\), the following data were obtained The order for the decomposition of AB is
1 0
2 1
3 2
4 1.5
Explanation:
Let rate equation be, \(\text { rate }=K[A B]^{\mathrm{n}}\) Case (1), \(2.75 \times 10^{-8}=\mathrm{k}[0.2]^{\mathrm{n}}\) Case (2), \(11 \times 10^{-8}=\mathrm{k}[0.40]^{\mathrm{n}}\) Case (3), \(24.75 \times 10^{-8}=\mathrm{k}[0.6]^{\mathrm{n}}\) Divided (2) by (1), \(\dfrac{11 \times 10^{-8}}{2.75 \times 10^{-8}}=\dfrac{[0.40]^{\mathrm{n}}}{[0.2]^{\mathrm{n}}} \Rightarrow 2^{\mathrm{n}}=4 \Rightarrow \mathrm{n}=2\) \(\therefore\) Order of reaction is 2 .
CHXII04:CHEMICAL KINETICS
320490
For a reaction \(\mathrm{A}+2 \mathrm{~B} \rightarrow\) Products, when concentration of \(\mathrm{B}\) alone is increased half life remains the same. If concentration of A alone is doubled, rate remains the same. The unit of rate constant of the reaction is
As \([' B ']\) increase, \(t_{\dfrac{1}{2}}\) remains same i.e. \(1^{\text {st }}\) order with respect to ' \(\mathrm{B}\) ' rate \(=\mathrm{k}[\mathrm{A}]^{0}[\mathrm{~B}]^{1}\) overall order \(=1\) \(\therefore\) units of \(\mathrm{k}=\mathrm{S}^{-1}\)
CHXII04:CHEMICAL KINETICS
320491
The half-lives of two samples are \(0.1 \mathrm{~s}\) and 0.8 s and their respective concentrations are \(400 \mathrm{~mol} \mathrm{~L}^{-1}\) and \(50 \mathrm{~mol} \mathrm{~L}^{-1}\). The order of the reaction is
320492
Using the data given below, the order and rate constant for the reaction: \(\mathrm{CH}_{3} \mathrm{CHO}(\mathrm{g}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{CO}(\mathrm{g})\) would be
320489
For the decomposition of a compound \(\mathrm{AB}\) at \(600 \mathrm{~K}\), the following data were obtained The order for the decomposition of AB is
1 0
2 1
3 2
4 1.5
Explanation:
Let rate equation be, \(\text { rate }=K[A B]^{\mathrm{n}}\) Case (1), \(2.75 \times 10^{-8}=\mathrm{k}[0.2]^{\mathrm{n}}\) Case (2), \(11 \times 10^{-8}=\mathrm{k}[0.40]^{\mathrm{n}}\) Case (3), \(24.75 \times 10^{-8}=\mathrm{k}[0.6]^{\mathrm{n}}\) Divided (2) by (1), \(\dfrac{11 \times 10^{-8}}{2.75 \times 10^{-8}}=\dfrac{[0.40]^{\mathrm{n}}}{[0.2]^{\mathrm{n}}} \Rightarrow 2^{\mathrm{n}}=4 \Rightarrow \mathrm{n}=2\) \(\therefore\) Order of reaction is 2 .
CHXII04:CHEMICAL KINETICS
320490
For a reaction \(\mathrm{A}+2 \mathrm{~B} \rightarrow\) Products, when concentration of \(\mathrm{B}\) alone is increased half life remains the same. If concentration of A alone is doubled, rate remains the same. The unit of rate constant of the reaction is
As \([' B ']\) increase, \(t_{\dfrac{1}{2}}\) remains same i.e. \(1^{\text {st }}\) order with respect to ' \(\mathrm{B}\) ' rate \(=\mathrm{k}[\mathrm{A}]^{0}[\mathrm{~B}]^{1}\) overall order \(=1\) \(\therefore\) units of \(\mathrm{k}=\mathrm{S}^{-1}\)
CHXII04:CHEMICAL KINETICS
320491
The half-lives of two samples are \(0.1 \mathrm{~s}\) and 0.8 s and their respective concentrations are \(400 \mathrm{~mol} \mathrm{~L}^{-1}\) and \(50 \mathrm{~mol} \mathrm{~L}^{-1}\). The order of the reaction is
320492
Using the data given below, the order and rate constant for the reaction: \(\mathrm{CH}_{3} \mathrm{CHO}(\mathrm{g}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{CO}(\mathrm{g})\) would be
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CHXII04:CHEMICAL KINETICS
320489
For the decomposition of a compound \(\mathrm{AB}\) at \(600 \mathrm{~K}\), the following data were obtained The order for the decomposition of AB is
1 0
2 1
3 2
4 1.5
Explanation:
Let rate equation be, \(\text { rate }=K[A B]^{\mathrm{n}}\) Case (1), \(2.75 \times 10^{-8}=\mathrm{k}[0.2]^{\mathrm{n}}\) Case (2), \(11 \times 10^{-8}=\mathrm{k}[0.40]^{\mathrm{n}}\) Case (3), \(24.75 \times 10^{-8}=\mathrm{k}[0.6]^{\mathrm{n}}\) Divided (2) by (1), \(\dfrac{11 \times 10^{-8}}{2.75 \times 10^{-8}}=\dfrac{[0.40]^{\mathrm{n}}}{[0.2]^{\mathrm{n}}} \Rightarrow 2^{\mathrm{n}}=4 \Rightarrow \mathrm{n}=2\) \(\therefore\) Order of reaction is 2 .
CHXII04:CHEMICAL KINETICS
320490
For a reaction \(\mathrm{A}+2 \mathrm{~B} \rightarrow\) Products, when concentration of \(\mathrm{B}\) alone is increased half life remains the same. If concentration of A alone is doubled, rate remains the same. The unit of rate constant of the reaction is
As \([' B ']\) increase, \(t_{\dfrac{1}{2}}\) remains same i.e. \(1^{\text {st }}\) order with respect to ' \(\mathrm{B}\) ' rate \(=\mathrm{k}[\mathrm{A}]^{0}[\mathrm{~B}]^{1}\) overall order \(=1\) \(\therefore\) units of \(\mathrm{k}=\mathrm{S}^{-1}\)
CHXII04:CHEMICAL KINETICS
320491
The half-lives of two samples are \(0.1 \mathrm{~s}\) and 0.8 s and their respective concentrations are \(400 \mathrm{~mol} \mathrm{~L}^{-1}\) and \(50 \mathrm{~mol} \mathrm{~L}^{-1}\). The order of the reaction is
320492
Using the data given below, the order and rate constant for the reaction: \(\mathrm{CH}_{3} \mathrm{CHO}(\mathrm{g}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{CO}(\mathrm{g})\) would be
