Rate of the Reaction
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CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
\(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{SO}_{3}(\mathrm{~g})\) is written as

1 \(\frac{{{\rm{\Delta }}\left[ {{\rm{S}}{{\rm{O}}_{\rm{2}}}} \right]}}{{{\rm{\Delta t}}}}\)
2 \(-\dfrac{\Delta\left[\mathrm{O}_{2}\right]}{\Delta \mathrm{t}}\)
3 \(\dfrac{1}{2} \dfrac{\Delta\left[\mathrm{SO}_{2}\right]}{\Delta \mathrm{t}}\)
4 \(\dfrac{\Delta\left[\mathrm{SO}_{3}\right]}{\Delta \mathrm{t}}\)
MHTCET - 2016
CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant
2 Rate \({\text{ = - }}\frac{{{\text{d}}\left[ {{{\text{C}}_{\text{2}}}{\text{ - }}{{\text{C}}_{\text{1}}}} \right]}}{{{{\text{t}}_{\text{2}}}{\text{ - }}{{\text{t}}_{\text{1}}}}}\)
3 Both (1) and (2)
4 It predicts the order of reaction
CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction \({\text{A + 2B}} \to {\text{C + 2D}}\), the initial rate \(\frac{{{\text{ - d[A]}}}}{{{\text{dt}}}}\) at \(\mathrm{t}=\) 0 was found to be \({\rm{2}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}{\rm{M}}{{\rm{s}}^{{\rm{ - 1}}}}\). What is the value of \(\frac{{{\text{ - d[B]}}}}{{{\text{dt}}}}{\mkern 1mu} {\mkern 1mu} {\text{at t = 0}}\,\,{\text{in M}}{{\text{s}}^{{\text{ - 1}}}}\) ?

1 \(2.6 \times 10^{-2}\)
2 \(5.2 \times 10^{-2}\)
3 \(1.3 \times 10^{-2}\)
4 \(1.0 \times 10^{-1}\)
CHXII04:CHEMICAL KINETICS

320580 For the reaction \({{\rm{N}}_{\rm{2}}}{\rm{(g) + 3}}{{\rm{H}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2N}}{{\rm{H}}_{\rm{3}}}{\rm{(g)}}\) under certain conditions of temperature and partial pressure of the reactants, the rate of formation of \({\text{N}}{{\text{H}}_{\text{3}}}{\mkern 1mu} {\mkern 1mu} {\text{is}}{\mkern 1mu} \,\,{\text{0}}{\text{.001}}\;{\text{mole}}{\mkern 1mu} {\mkern 1mu} {\text{h}}{{\text{r}}^{{\text{ - 1}}}}\). The rate of conversion of \(\mathrm{H}_{2}\) under the same conditions is

1 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
2 \({\rm{0}}{\rm{.0015}}\;{\rm{mole}}\,\,{\rm{hr}}\)
3 \({\rm{1}}{\rm{.52 \times 1}}{{\rm{0}}^{\rm{4}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
4 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 14}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
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CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
\(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{SO}_{3}(\mathrm{~g})\) is written as

1 \(\frac{{{\rm{\Delta }}\left[ {{\rm{S}}{{\rm{O}}_{\rm{2}}}} \right]}}{{{\rm{\Delta t}}}}\)
2 \(-\dfrac{\Delta\left[\mathrm{O}_{2}\right]}{\Delta \mathrm{t}}\)
3 \(\dfrac{1}{2} \dfrac{\Delta\left[\mathrm{SO}_{2}\right]}{\Delta \mathrm{t}}\)
4 \(\dfrac{\Delta\left[\mathrm{SO}_{3}\right]}{\Delta \mathrm{t}}\)
MHTCET - 2016
CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant
2 Rate \({\text{ = - }}\frac{{{\text{d}}\left[ {{{\text{C}}_{\text{2}}}{\text{ - }}{{\text{C}}_{\text{1}}}} \right]}}{{{{\text{t}}_{\text{2}}}{\text{ - }}{{\text{t}}_{\text{1}}}}}\)
3 Both (1) and (2)
4 It predicts the order of reaction
CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction \({\text{A + 2B}} \to {\text{C + 2D}}\), the initial rate \(\frac{{{\text{ - d[A]}}}}{{{\text{dt}}}}\) at \(\mathrm{t}=\) 0 was found to be \({\rm{2}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}{\rm{M}}{{\rm{s}}^{{\rm{ - 1}}}}\). What is the value of \(\frac{{{\text{ - d[B]}}}}{{{\text{dt}}}}{\mkern 1mu} {\mkern 1mu} {\text{at t = 0}}\,\,{\text{in M}}{{\text{s}}^{{\text{ - 1}}}}\) ?

1 \(2.6 \times 10^{-2}\)
2 \(5.2 \times 10^{-2}\)
3 \(1.3 \times 10^{-2}\)
4 \(1.0 \times 10^{-1}\)
CHXII04:CHEMICAL KINETICS

320580 For the reaction \({{\rm{N}}_{\rm{2}}}{\rm{(g) + 3}}{{\rm{H}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2N}}{{\rm{H}}_{\rm{3}}}{\rm{(g)}}\) under certain conditions of temperature and partial pressure of the reactants, the rate of formation of \({\text{N}}{{\text{H}}_{\text{3}}}{\mkern 1mu} {\mkern 1mu} {\text{is}}{\mkern 1mu} \,\,{\text{0}}{\text{.001}}\;{\text{mole}}{\mkern 1mu} {\mkern 1mu} {\text{h}}{{\text{r}}^{{\text{ - 1}}}}\). The rate of conversion of \(\mathrm{H}_{2}\) under the same conditions is

1 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
2 \({\rm{0}}{\rm{.0015}}\;{\rm{mole}}\,\,{\rm{hr}}\)
3 \({\rm{1}}{\rm{.52 \times 1}}{{\rm{0}}^{\rm{4}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
4 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 14}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
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CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
\(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{SO}_{3}(\mathrm{~g})\) is written as

1 \(\frac{{{\rm{\Delta }}\left[ {{\rm{S}}{{\rm{O}}_{\rm{2}}}} \right]}}{{{\rm{\Delta t}}}}\)
2 \(-\dfrac{\Delta\left[\mathrm{O}_{2}\right]}{\Delta \mathrm{t}}\)
3 \(\dfrac{1}{2} \dfrac{\Delta\left[\mathrm{SO}_{2}\right]}{\Delta \mathrm{t}}\)
4 \(\dfrac{\Delta\left[\mathrm{SO}_{3}\right]}{\Delta \mathrm{t}}\)
MHTCET - 2016
CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant
2 Rate \({\text{ = - }}\frac{{{\text{d}}\left[ {{{\text{C}}_{\text{2}}}{\text{ - }}{{\text{C}}_{\text{1}}}} \right]}}{{{{\text{t}}_{\text{2}}}{\text{ - }}{{\text{t}}_{\text{1}}}}}\)
3 Both (1) and (2)
4 It predicts the order of reaction
CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction \({\text{A + 2B}} \to {\text{C + 2D}}\), the initial rate \(\frac{{{\text{ - d[A]}}}}{{{\text{dt}}}}\) at \(\mathrm{t}=\) 0 was found to be \({\rm{2}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}{\rm{M}}{{\rm{s}}^{{\rm{ - 1}}}}\). What is the value of \(\frac{{{\text{ - d[B]}}}}{{{\text{dt}}}}{\mkern 1mu} {\mkern 1mu} {\text{at t = 0}}\,\,{\text{in M}}{{\text{s}}^{{\text{ - 1}}}}\) ?

1 \(2.6 \times 10^{-2}\)
2 \(5.2 \times 10^{-2}\)
3 \(1.3 \times 10^{-2}\)
4 \(1.0 \times 10^{-1}\)
CHXII04:CHEMICAL KINETICS

320580 For the reaction \({{\rm{N}}_{\rm{2}}}{\rm{(g) + 3}}{{\rm{H}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2N}}{{\rm{H}}_{\rm{3}}}{\rm{(g)}}\) under certain conditions of temperature and partial pressure of the reactants, the rate of formation of \({\text{N}}{{\text{H}}_{\text{3}}}{\mkern 1mu} {\mkern 1mu} {\text{is}}{\mkern 1mu} \,\,{\text{0}}{\text{.001}}\;{\text{mole}}{\mkern 1mu} {\mkern 1mu} {\text{h}}{{\text{r}}^{{\text{ - 1}}}}\). The rate of conversion of \(\mathrm{H}_{2}\) under the same conditions is

1 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
2 \({\rm{0}}{\rm{.0015}}\;{\rm{mole}}\,\,{\rm{hr}}\)
3 \({\rm{1}}{\rm{.52 \times 1}}{{\rm{0}}^{\rm{4}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
4 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 14}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
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CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
\(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{SO}_{3}(\mathrm{~g})\) is written as

1 \(\frac{{{\rm{\Delta }}\left[ {{\rm{S}}{{\rm{O}}_{\rm{2}}}} \right]}}{{{\rm{\Delta t}}}}\)
2 \(-\dfrac{\Delta\left[\mathrm{O}_{2}\right]}{\Delta \mathrm{t}}\)
3 \(\dfrac{1}{2} \dfrac{\Delta\left[\mathrm{SO}_{2}\right]}{\Delta \mathrm{t}}\)
4 \(\dfrac{\Delta\left[\mathrm{SO}_{3}\right]}{\Delta \mathrm{t}}\)
MHTCET - 2016
CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant
2 Rate \({\text{ = - }}\frac{{{\text{d}}\left[ {{{\text{C}}_{\text{2}}}{\text{ - }}{{\text{C}}_{\text{1}}}} \right]}}{{{{\text{t}}_{\text{2}}}{\text{ - }}{{\text{t}}_{\text{1}}}}}\)
3 Both (1) and (2)
4 It predicts the order of reaction
CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction \({\text{A + 2B}} \to {\text{C + 2D}}\), the initial rate \(\frac{{{\text{ - d[A]}}}}{{{\text{dt}}}}\) at \(\mathrm{t}=\) 0 was found to be \({\rm{2}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}{\rm{M}}{{\rm{s}}^{{\rm{ - 1}}}}\). What is the value of \(\frac{{{\text{ - d[B]}}}}{{{\text{dt}}}}{\mkern 1mu} {\mkern 1mu} {\text{at t = 0}}\,\,{\text{in M}}{{\text{s}}^{{\text{ - 1}}}}\) ?

1 \(2.6 \times 10^{-2}\)
2 \(5.2 \times 10^{-2}\)
3 \(1.3 \times 10^{-2}\)
4 \(1.0 \times 10^{-1}\)
CHXII04:CHEMICAL KINETICS

320580 For the reaction \({{\rm{N}}_{\rm{2}}}{\rm{(g) + 3}}{{\rm{H}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2N}}{{\rm{H}}_{\rm{3}}}{\rm{(g)}}\) under certain conditions of temperature and partial pressure of the reactants, the rate of formation of \({\text{N}}{{\text{H}}_{\text{3}}}{\mkern 1mu} {\mkern 1mu} {\text{is}}{\mkern 1mu} \,\,{\text{0}}{\text{.001}}\;{\text{mole}}{\mkern 1mu} {\mkern 1mu} {\text{h}}{{\text{r}}^{{\text{ - 1}}}}\). The rate of conversion of \(\mathrm{H}_{2}\) under the same conditions is

1 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
2 \({\rm{0}}{\rm{.0015}}\;{\rm{mole}}\,\,{\rm{hr}}\)
3 \({\rm{1}}{\rm{.52 \times 1}}{{\rm{0}}^{\rm{4}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
4 \({\rm{1}}{\rm{.82 \times 1}}{{\rm{0}}^{{\rm{ - 14}}}}{\rm{mole}}{\mkern 1mu} {\mkern 1mu} {\rm{hr}}\)
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