320506 The rates of a certain reaction \((\mathrm{dc} / \mathrm{dt})\) at different times are as follows?
\(\begin{array}{*{20}{c}}{{\rm{Time}}}&{{\rm{Rate}}\,{\rm{(mole}}\,\,{\rm{lite}}{{\rm{r}}^{{\rm{ - 1}}}}\,{\rm{se}}{{\rm{c}}^{{\rm{ - 1}}}}{\rm{)}}}\\{\rm{0}}&{{\rm{2}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{10}}}&{{\rm{2}}{\rm{.78 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{20}}}&{{\rm{2}}{\rm{.81 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{30}}}&{{\rm{2}}{\rm{.79 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\end{array}\)
The reaction is

320507 For the reaction \(\mathrm{aA} \rightarrow \mathrm{xP}\) when \({\text{[A] = 2}}{\text{.2 mM}}\) the rate was found to be \({\text{2}}{\text{.4 m M}}{{\text{s}}^{{\text{ - 1}}}}\). On reducing the concentration of A to half, the rate changes to \({\text{0}}{\text{.6 mM}}{{\text{s}}^{{\text{ - 1}}}}\). The order of reaction with respect to \(\mathrm{A}\) is

320508 A student has studied the decomposition of a gas \(\mathrm{AB}_{3}\) at \(25^{\circ} \mathrm{C}\). He obtained the following data.


The order of the reaction is

320509 The following results were obtained during kinetic studies of the reaction; \(2 A+B \rightarrow\) products
The time (in minutes) required to consume half of \(A\) is

320506 The rates of a certain reaction \((\mathrm{dc} / \mathrm{dt})\) at different times are as follows?
\(\begin{array}{*{20}{c}}{{\rm{Time}}}&{{\rm{Rate}}\,{\rm{(mole}}\,\,{\rm{lite}}{{\rm{r}}^{{\rm{ - 1}}}}\,{\rm{se}}{{\rm{c}}^{{\rm{ - 1}}}}{\rm{)}}}\\{\rm{0}}&{{\rm{2}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{10}}}&{{\rm{2}}{\rm{.78 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{20}}}&{{\rm{2}}{\rm{.81 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{30}}}&{{\rm{2}}{\rm{.79 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\end{array}\)
The reaction is

320507 For the reaction \(\mathrm{aA} \rightarrow \mathrm{xP}\) when \({\text{[A] = 2}}{\text{.2 mM}}\) the rate was found to be \({\text{2}}{\text{.4 m M}}{{\text{s}}^{{\text{ - 1}}}}\). On reducing the concentration of A to half, the rate changes to \({\text{0}}{\text{.6 mM}}{{\text{s}}^{{\text{ - 1}}}}\). The order of reaction with respect to \(\mathrm{A}\) is

320508 A student has studied the decomposition of a gas \(\mathrm{AB}_{3}\) at \(25^{\circ} \mathrm{C}\). He obtained the following data.


The order of the reaction is

320509 The following results were obtained during kinetic studies of the reaction; \(2 A+B \rightarrow\) products
The time (in minutes) required to consume half of \(A\) is

320506 The rates of a certain reaction \((\mathrm{dc} / \mathrm{dt})\) at different times are as follows?
\(\begin{array}{*{20}{c}}{{\rm{Time}}}&{{\rm{Rate}}\,{\rm{(mole}}\,\,{\rm{lite}}{{\rm{r}}^{{\rm{ - 1}}}}\,{\rm{se}}{{\rm{c}}^{{\rm{ - 1}}}}{\rm{)}}}\\{\rm{0}}&{{\rm{2}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{10}}}&{{\rm{2}}{\rm{.78 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{20}}}&{{\rm{2}}{\rm{.81 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{30}}}&{{\rm{2}}{\rm{.79 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\end{array}\)
The reaction is

320507 For the reaction \(\mathrm{aA} \rightarrow \mathrm{xP}\) when \({\text{[A] = 2}}{\text{.2 mM}}\) the rate was found to be \({\text{2}}{\text{.4 m M}}{{\text{s}}^{{\text{ - 1}}}}\). On reducing the concentration of A to half, the rate changes to \({\text{0}}{\text{.6 mM}}{{\text{s}}^{{\text{ - 1}}}}\). The order of reaction with respect to \(\mathrm{A}\) is

320508 A student has studied the decomposition of a gas \(\mathrm{AB}_{3}\) at \(25^{\circ} \mathrm{C}\). He obtained the following data.


The order of the reaction is

320509 The following results were obtained during kinetic studies of the reaction; \(2 A+B \rightarrow\) products
The time (in minutes) required to consume half of \(A\) is

320506 The rates of a certain reaction \((\mathrm{dc} / \mathrm{dt})\) at different times are as follows?
\(\begin{array}{*{20}{c}}{{\rm{Time}}}&{{\rm{Rate}}\,{\rm{(mole}}\,\,{\rm{lite}}{{\rm{r}}^{{\rm{ - 1}}}}\,{\rm{se}}{{\rm{c}}^{{\rm{ - 1}}}}{\rm{)}}}\\{\rm{0}}&{{\rm{2}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{10}}}&{{\rm{2}}{\rm{.78 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{20}}}&{{\rm{2}}{\rm{.81 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\\{{\rm{30}}}&{{\rm{2}}{\rm{.79 \times 1}}{{\rm{0}}^{{\rm{ - 2}}}}}\end{array}\)
The reaction is

320507 For the reaction \(\mathrm{aA} \rightarrow \mathrm{xP}\) when \({\text{[A] = 2}}{\text{.2 mM}}\) the rate was found to be \({\text{2}}{\text{.4 m M}}{{\text{s}}^{{\text{ - 1}}}}\). On reducing the concentration of A to half, the rate changes to \({\text{0}}{\text{.6 mM}}{{\text{s}}^{{\text{ - 1}}}}\). The order of reaction with respect to \(\mathrm{A}\) is

320508 A student has studied the decomposition of a gas \(\mathrm{AB}_{3}\) at \(25^{\circ} \mathrm{C}\). He obtained the following data.


The order of the reaction is

320509 The following results were obtained during kinetic studies of the reaction; \(2 A+B \rightarrow\) products
The time (in minutes) required to consume half of \(A\) is