Dependence of Rate on Concentration
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CHXII04:CHEMICAL KINETICS

320150 The rate constant of the reaction \({\rm{2}}{{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{(aq)}} \to {\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O(l) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\)

At what concentration of \({{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{,the}}\,\,{\rm{rate}}\,\,{\rm{of}}\,\,{\rm{reaction}}\,\,{\rm{will}}\,\,{\rm{be}}{\mkern 1mu} {\mkern 1mu} \,{\rm{2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}\,{\rm{M}}\,{{\rm{s}}^{{\rm{ - 1}}}}\)

1 \(6.67 \times 10^{-3} M\)
2 \(2 \mathrm{M}\)
3 \(4 \mathrm{M}\)
4 \(0.08 \mathrm{M}\)
CHXII04:CHEMICAL KINETICS

320151 The unit of rate constant for a zero order reaction is

1 \(({\rm{mol}}\,\,{{\rm{L}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
2 \(({\rm{L}}\,\,{\rm{mo}}{{\rm{l}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
3 \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\)
4 \(\mathrm{s}^{-1}\)
CHXII04:CHEMICAL KINETICS

320152 Which of the following " k " values represents the fastest reaction?

1 \(1.5 \times 10^{-3}\)
2 \(9.2 \times 10^{-6}\)
3 \(5.5 \times 10^{-4}\)
4 \(2.39 \times 10^{-8}\)
CHXII04:CHEMICAL KINETICS

320153 For reaction, \(2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}\), the rate equation can be expressed in two ways \(-\dfrac{\mathrm{d}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]\) and \(+\dfrac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}=\mathrm{k}^{\prime}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right] . \mathrm{k}\) and \(\mathrm{k}^{\prime}\) are related

1 \(\mathrm{k}=4 \mathrm{k}^{\prime}\)
2 \(\mathrm{k}=2 \mathrm{k}^{\prime}\)
3 \(2 \mathrm{k}=\mathrm{k}^{\prime}\)
4 \(\mathrm{k}=\mathrm{k}^{\prime}\)
JEE - 2014
NEET DIGITAL LIBRARY
CHXII04:CHEMICAL KINETICS

320150 The rate constant of the reaction \({\rm{2}}{{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{(aq)}} \to {\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O(l) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\)

At what concentration of \({{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{,the}}\,\,{\rm{rate}}\,\,{\rm{of}}\,\,{\rm{reaction}}\,\,{\rm{will}}\,\,{\rm{be}}{\mkern 1mu} {\mkern 1mu} \,{\rm{2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}\,{\rm{M}}\,{{\rm{s}}^{{\rm{ - 1}}}}\)

1 \(6.67 \times 10^{-3} M\)
2 \(2 \mathrm{M}\)
3 \(4 \mathrm{M}\)
4 \(0.08 \mathrm{M}\)
CHXII04:CHEMICAL KINETICS

320151 The unit of rate constant for a zero order reaction is

1 \(({\rm{mol}}\,\,{{\rm{L}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
2 \(({\rm{L}}\,\,{\rm{mo}}{{\rm{l}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
3 \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\)
4 \(\mathrm{s}^{-1}\)
CHXII04:CHEMICAL KINETICS

320152 Which of the following " k " values represents the fastest reaction?

1 \(1.5 \times 10^{-3}\)
2 \(9.2 \times 10^{-6}\)
3 \(5.5 \times 10^{-4}\)
4 \(2.39 \times 10^{-8}\)
CHXII04:CHEMICAL KINETICS

320153 For reaction, \(2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}\), the rate equation can be expressed in two ways \(-\dfrac{\mathrm{d}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]\) and \(+\dfrac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}=\mathrm{k}^{\prime}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right] . \mathrm{k}\) and \(\mathrm{k}^{\prime}\) are related

1 \(\mathrm{k}=4 \mathrm{k}^{\prime}\)
2 \(\mathrm{k}=2 \mathrm{k}^{\prime}\)
3 \(2 \mathrm{k}=\mathrm{k}^{\prime}\)
4 \(\mathrm{k}=\mathrm{k}^{\prime}\)
JEE - 2014
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CHXII04:CHEMICAL KINETICS

320150 The rate constant of the reaction \({\rm{2}}{{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{(aq)}} \to {\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O(l) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\)

At what concentration of \({{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{,the}}\,\,{\rm{rate}}\,\,{\rm{of}}\,\,{\rm{reaction}}\,\,{\rm{will}}\,\,{\rm{be}}{\mkern 1mu} {\mkern 1mu} \,{\rm{2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}\,{\rm{M}}\,{{\rm{s}}^{{\rm{ - 1}}}}\)

1 \(6.67 \times 10^{-3} M\)
2 \(2 \mathrm{M}\)
3 \(4 \mathrm{M}\)
4 \(0.08 \mathrm{M}\)
CHXII04:CHEMICAL KINETICS

320151 The unit of rate constant for a zero order reaction is

1 \(({\rm{mol}}\,\,{{\rm{L}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
2 \(({\rm{L}}\,\,{\rm{mo}}{{\rm{l}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
3 \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\)
4 \(\mathrm{s}^{-1}\)
CHXII04:CHEMICAL KINETICS

320152 Which of the following " k " values represents the fastest reaction?

1 \(1.5 \times 10^{-3}\)
2 \(9.2 \times 10^{-6}\)
3 \(5.5 \times 10^{-4}\)
4 \(2.39 \times 10^{-8}\)
CHXII04:CHEMICAL KINETICS

320153 For reaction, \(2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}\), the rate equation can be expressed in two ways \(-\dfrac{\mathrm{d}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]\) and \(+\dfrac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}=\mathrm{k}^{\prime}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right] . \mathrm{k}\) and \(\mathrm{k}^{\prime}\) are related

1 \(\mathrm{k}=4 \mathrm{k}^{\prime}\)
2 \(\mathrm{k}=2 \mathrm{k}^{\prime}\)
3 \(2 \mathrm{k}=\mathrm{k}^{\prime}\)
4 \(\mathrm{k}=\mathrm{k}^{\prime}\)
JEE - 2014
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CHXII04:CHEMICAL KINETICS

320150 The rate constant of the reaction \({\rm{2}}{{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{(aq)}} \to {\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O(l) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\)

At what concentration of \({{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}{\rm{,the}}\,\,{\rm{rate}}\,\,{\rm{of}}\,\,{\rm{reaction}}\,\,{\rm{will}}\,\,{\rm{be}}{\mkern 1mu} {\mkern 1mu} \,{\rm{2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}\,{\rm{M}}\,{{\rm{s}}^{{\rm{ - 1}}}}\)

1 \(6.67 \times 10^{-3} M\)
2 \(2 \mathrm{M}\)
3 \(4 \mathrm{M}\)
4 \(0.08 \mathrm{M}\)
CHXII04:CHEMICAL KINETICS

320151 The unit of rate constant for a zero order reaction is

1 \(({\rm{mol}}\,\,{{\rm{L}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
2 \(({\rm{L}}\,\,{\rm{mo}}{{\rm{l}}^{ - 1}}\;{{\rm{s}}^{ - 1}})\)
3 \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\)
4 \(\mathrm{s}^{-1}\)
CHXII04:CHEMICAL KINETICS

320152 Which of the following " k " values represents the fastest reaction?

1 \(1.5 \times 10^{-3}\)
2 \(9.2 \times 10^{-6}\)
3 \(5.5 \times 10^{-4}\)
4 \(2.39 \times 10^{-8}\)
CHXII04:CHEMICAL KINETICS

320153 For reaction, \(2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}\), the rate equation can be expressed in two ways \(-\dfrac{\mathrm{d}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]\) and \(+\dfrac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}=\mathrm{k}^{\prime}\left[\mathrm{N}_{2} \mathrm{O}_{5}\right] . \mathrm{k}\) and \(\mathrm{k}^{\prime}\) are related

1 \(\mathrm{k}=4 \mathrm{k}^{\prime}\)
2 \(\mathrm{k}=2 \mathrm{k}^{\prime}\)
3 \(2 \mathrm{k}=\mathrm{k}^{\prime}\)
4 \(\mathrm{k}=\mathrm{k}^{\prime}\)
JEE - 2014
NEET DIGITAL LIBRARY