320146
The rate constant of the reaction \({\mathrm{A \longrightarrow B}}\) is \({\mathrm{1.0 \times 10^{-4} \mathrm{M} \mathrm{s}^{-1}}}\). After 100 min , if the concentration of A is 4.40 M , then concentration of \({\mathrm{B}}\) will be ____ M .
1 0.44
2 4.4
3 5
4 0.6
Explanation:
For the reaction, \({\mathrm{\mathrm{A} \longrightarrow \mathrm{B}}}\) \({\mathrm{\mathrm{k}=1 \times 10^{-4} \,\mathrm{M} \mathrm{s}^{-1}}}\) \({\mathrm{\therefore}}\) Since the units of k is M \({{\rm{s}}^{ - 1}}\), it is a zero order reaction. \({\mathrm{\therefore k=\dfrac{[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}}{\mathrm{t}}}}\) \({\mathrm{\therefore \mathrm{t}=100 \mathrm{~min}=6000 \mathrm{~s}}}\) \({\mathrm{\therefore 1 \times 10^{-4}=\dfrac{[\mathrm{A}]_{0}-4.40}{6000}}}\) \(\begin{aligned}& {[\mathrm{A}]_{0}=5.00 \mathrm{M}} \\& {[\mathrm{B}]_{\mathrm{t}}=[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}=5.00-4.40=0.60 \mathrm{M}}\end{aligned}\)
CHXII04:CHEMICAL KINETICS
320147
Assertion : Rate of reaction doubles when concentration of reactant is doubled if it is a first order reaction. Reason : Rate constant also doubles.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For a given reaction, rate constant is constant and independent of the concentration of reactant. For first order raection : \(\mathrm{r}_{1}=\mathrm{K}[\mathrm{R}]\) According to equation, \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) \(\mathrm{r}_{2}=\mathrm{k}\left[\mathrm{R}_{2}\right] \Rightarrow \mathrm{r}_{2}=\mathrm{k}\left[2 \mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{k}\left[\mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) Rate constants depends only on temperature not on concentrations. So option (3) is correct.
CHXII04:CHEMICAL KINETICS
320148
The rate of reaction: \(2 \mathrm{NO}+\mathrm{Cl}_{2} \rightarrow 2 \mathrm{NOCl}\) is given by the rate, equation rate \({\rm{ = k[NO}}{{\rm{]}}^{\rm{2}}}\left[ {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right]\). The value of the rate constant can be increased by
1 Increasing the concentration of the \(\mathrm{Cl}_{2}\)
2 Increasing the concentration of \(\mathrm{NO}\)
3 Increasing the temperature
4 Doing all of these
Explanation:
\(15 \mathrm{k}\) increases with increase in temperature
CHXII04:CHEMICAL KINETICS
320149
The rate constant is numerically the same for three reaction of first, second and third order respectively. Which one is true for rate of three reaction, if concentration of reactant is greater than \(1 \mathrm{M}\) ?
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CHXII04:CHEMICAL KINETICS
320146
The rate constant of the reaction \({\mathrm{A \longrightarrow B}}\) is \({\mathrm{1.0 \times 10^{-4} \mathrm{M} \mathrm{s}^{-1}}}\). After 100 min , if the concentration of A is 4.40 M , then concentration of \({\mathrm{B}}\) will be ____ M .
1 0.44
2 4.4
3 5
4 0.6
Explanation:
For the reaction, \({\mathrm{\mathrm{A} \longrightarrow \mathrm{B}}}\) \({\mathrm{\mathrm{k}=1 \times 10^{-4} \,\mathrm{M} \mathrm{s}^{-1}}}\) \({\mathrm{\therefore}}\) Since the units of k is M \({{\rm{s}}^{ - 1}}\), it is a zero order reaction. \({\mathrm{\therefore k=\dfrac{[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}}{\mathrm{t}}}}\) \({\mathrm{\therefore \mathrm{t}=100 \mathrm{~min}=6000 \mathrm{~s}}}\) \({\mathrm{\therefore 1 \times 10^{-4}=\dfrac{[\mathrm{A}]_{0}-4.40}{6000}}}\) \(\begin{aligned}& {[\mathrm{A}]_{0}=5.00 \mathrm{M}} \\& {[\mathrm{B}]_{\mathrm{t}}=[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}=5.00-4.40=0.60 \mathrm{M}}\end{aligned}\)
CHXII04:CHEMICAL KINETICS
320147
Assertion : Rate of reaction doubles when concentration of reactant is doubled if it is a first order reaction. Reason : Rate constant also doubles.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For a given reaction, rate constant is constant and independent of the concentration of reactant. For first order raection : \(\mathrm{r}_{1}=\mathrm{K}[\mathrm{R}]\) According to equation, \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) \(\mathrm{r}_{2}=\mathrm{k}\left[\mathrm{R}_{2}\right] \Rightarrow \mathrm{r}_{2}=\mathrm{k}\left[2 \mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{k}\left[\mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) Rate constants depends only on temperature not on concentrations. So option (3) is correct.
CHXII04:CHEMICAL KINETICS
320148
The rate of reaction: \(2 \mathrm{NO}+\mathrm{Cl}_{2} \rightarrow 2 \mathrm{NOCl}\) is given by the rate, equation rate \({\rm{ = k[NO}}{{\rm{]}}^{\rm{2}}}\left[ {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right]\). The value of the rate constant can be increased by
1 Increasing the concentration of the \(\mathrm{Cl}_{2}\)
2 Increasing the concentration of \(\mathrm{NO}\)
3 Increasing the temperature
4 Doing all of these
Explanation:
\(15 \mathrm{k}\) increases with increase in temperature
CHXII04:CHEMICAL KINETICS
320149
The rate constant is numerically the same for three reaction of first, second and third order respectively. Which one is true for rate of three reaction, if concentration of reactant is greater than \(1 \mathrm{M}\) ?
320146
The rate constant of the reaction \({\mathrm{A \longrightarrow B}}\) is \({\mathrm{1.0 \times 10^{-4} \mathrm{M} \mathrm{s}^{-1}}}\). After 100 min , if the concentration of A is 4.40 M , then concentration of \({\mathrm{B}}\) will be ____ M .
1 0.44
2 4.4
3 5
4 0.6
Explanation:
For the reaction, \({\mathrm{\mathrm{A} \longrightarrow \mathrm{B}}}\) \({\mathrm{\mathrm{k}=1 \times 10^{-4} \,\mathrm{M} \mathrm{s}^{-1}}}\) \({\mathrm{\therefore}}\) Since the units of k is M \({{\rm{s}}^{ - 1}}\), it is a zero order reaction. \({\mathrm{\therefore k=\dfrac{[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}}{\mathrm{t}}}}\) \({\mathrm{\therefore \mathrm{t}=100 \mathrm{~min}=6000 \mathrm{~s}}}\) \({\mathrm{\therefore 1 \times 10^{-4}=\dfrac{[\mathrm{A}]_{0}-4.40}{6000}}}\) \(\begin{aligned}& {[\mathrm{A}]_{0}=5.00 \mathrm{M}} \\& {[\mathrm{B}]_{\mathrm{t}}=[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}=5.00-4.40=0.60 \mathrm{M}}\end{aligned}\)
CHXII04:CHEMICAL KINETICS
320147
Assertion : Rate of reaction doubles when concentration of reactant is doubled if it is a first order reaction. Reason : Rate constant also doubles.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For a given reaction, rate constant is constant and independent of the concentration of reactant. For first order raection : \(\mathrm{r}_{1}=\mathrm{K}[\mathrm{R}]\) According to equation, \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) \(\mathrm{r}_{2}=\mathrm{k}\left[\mathrm{R}_{2}\right] \Rightarrow \mathrm{r}_{2}=\mathrm{k}\left[2 \mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{k}\left[\mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) Rate constants depends only on temperature not on concentrations. So option (3) is correct.
CHXII04:CHEMICAL KINETICS
320148
The rate of reaction: \(2 \mathrm{NO}+\mathrm{Cl}_{2} \rightarrow 2 \mathrm{NOCl}\) is given by the rate, equation rate \({\rm{ = k[NO}}{{\rm{]}}^{\rm{2}}}\left[ {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right]\). The value of the rate constant can be increased by
1 Increasing the concentration of the \(\mathrm{Cl}_{2}\)
2 Increasing the concentration of \(\mathrm{NO}\)
3 Increasing the temperature
4 Doing all of these
Explanation:
\(15 \mathrm{k}\) increases with increase in temperature
CHXII04:CHEMICAL KINETICS
320149
The rate constant is numerically the same for three reaction of first, second and third order respectively. Which one is true for rate of three reaction, if concentration of reactant is greater than \(1 \mathrm{M}\) ?
320146
The rate constant of the reaction \({\mathrm{A \longrightarrow B}}\) is \({\mathrm{1.0 \times 10^{-4} \mathrm{M} \mathrm{s}^{-1}}}\). After 100 min , if the concentration of A is 4.40 M , then concentration of \({\mathrm{B}}\) will be ____ M .
1 0.44
2 4.4
3 5
4 0.6
Explanation:
For the reaction, \({\mathrm{\mathrm{A} \longrightarrow \mathrm{B}}}\) \({\mathrm{\mathrm{k}=1 \times 10^{-4} \,\mathrm{M} \mathrm{s}^{-1}}}\) \({\mathrm{\therefore}}\) Since the units of k is M \({{\rm{s}}^{ - 1}}\), it is a zero order reaction. \({\mathrm{\therefore k=\dfrac{[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}}{\mathrm{t}}}}\) \({\mathrm{\therefore \mathrm{t}=100 \mathrm{~min}=6000 \mathrm{~s}}}\) \({\mathrm{\therefore 1 \times 10^{-4}=\dfrac{[\mathrm{A}]_{0}-4.40}{6000}}}\) \(\begin{aligned}& {[\mathrm{A}]_{0}=5.00 \mathrm{M}} \\& {[\mathrm{B}]_{\mathrm{t}}=[\mathrm{A}]_{0}-[\mathrm{A}]_{\mathrm{t}}=5.00-4.40=0.60 \mathrm{M}}\end{aligned}\)
CHXII04:CHEMICAL KINETICS
320147
Assertion : Rate of reaction doubles when concentration of reactant is doubled if it is a first order reaction. Reason : Rate constant also doubles.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For a given reaction, rate constant is constant and independent of the concentration of reactant. For first order raection : \(\mathrm{r}_{1}=\mathrm{K}[\mathrm{R}]\) According to equation, \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) \(\mathrm{r}_{2}=\mathrm{k}\left[\mathrm{R}_{2}\right] \Rightarrow \mathrm{r}_{2}=\mathrm{k}\left[2 \mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{k}\left[\mathrm{R}_{1}\right]\) \(\mathrm{r}_{2}=2 \mathrm{r}_{1}\) Rate constants depends only on temperature not on concentrations. So option (3) is correct.
CHXII04:CHEMICAL KINETICS
320148
The rate of reaction: \(2 \mathrm{NO}+\mathrm{Cl}_{2} \rightarrow 2 \mathrm{NOCl}\) is given by the rate, equation rate \({\rm{ = k[NO}}{{\rm{]}}^{\rm{2}}}\left[ {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right]\). The value of the rate constant can be increased by
1 Increasing the concentration of the \(\mathrm{Cl}_{2}\)
2 Increasing the concentration of \(\mathrm{NO}\)
3 Increasing the temperature
4 Doing all of these
Explanation:
\(15 \mathrm{k}\) increases with increase in temperature
CHXII04:CHEMICAL KINETICS
320149
The rate constant is numerically the same for three reaction of first, second and third order respectively. Which one is true for rate of three reaction, if concentration of reactant is greater than \(1 \mathrm{M}\) ?