320510 What is the order of a chemical reaction \({\rm{A + 2B}}\mathop \to \limits^k {\rm{C}}\), if the rate of formation of C increases by a factor of 2.82 on doubling the concentration of A and increases by a factor of 9 on tripling the concentration of B ?

320511 If \(50 \%\) of a reaction occurs in 100 seconds and \(75 \%\) of the reaction occurs in 200 seconds, the order of this reaction is:

320512 The experimental data for the reaction,
\({\rm{2A + }}{{\rm{B}}_{\rm{2}}} \to {\rm{2AB,}}\,\,{\rm{is }}\)
\(\begin{array}{*{20}{c}}\begin{array}{l}{\rm{Expt}}\\\,\,{\rm{No}}{\rm{.}}\end{array}&{\left[ {\rm{A}} \right]}&{\left[ {{{\rm{B}}_{\rm{2}}}} \right]}&{{\rm{Rate}}\,\,{\rm{(}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}}\\{{\rm{1}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{2}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{3}}{\rm{.}}}&{{\rm{1}}{\rm{.0}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\end{array}\)
The rate equation for the above data is

320513 For the decomposition of HI at \(1000 \mathrm{~K}\), the following data were obtained

[HI] M Rate of decomposition of HI (mole \(L^{-1} \mathrm{~s}^{-1}\) )

\(0.1 \quad 2.75 \times 10^{-8}\)

\(0.2 \quad 11 \times 10^{-8}\)

\(0.3 \quad 24.75 \times 10^{-8}\)

The order of reaction is:

320514 At \(518^{\circ} \mathrm{C}\), the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 Torr \({{\text{s}}^{{\text{ - 1}}}}\) when 5% had reacted and 0.5 torr \({{\text{s}}^{{\text{ - 1}}}}\) when 33% had reacted. The order of the reaction is :

320510 What is the order of a chemical reaction \({\rm{A + 2B}}\mathop \to \limits^k {\rm{C}}\), if the rate of formation of C increases by a factor of 2.82 on doubling the concentration of A and increases by a factor of 9 on tripling the concentration of B ?

320511 If \(50 \%\) of a reaction occurs in 100 seconds and \(75 \%\) of the reaction occurs in 200 seconds, the order of this reaction is:

320512 The experimental data for the reaction,
\({\rm{2A + }}{{\rm{B}}_{\rm{2}}} \to {\rm{2AB,}}\,\,{\rm{is }}\)
\(\begin{array}{*{20}{c}}\begin{array}{l}{\rm{Expt}}\\\,\,{\rm{No}}{\rm{.}}\end{array}&{\left[ {\rm{A}} \right]}&{\left[ {{{\rm{B}}_{\rm{2}}}} \right]}&{{\rm{Rate}}\,\,{\rm{(}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}}\\{{\rm{1}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{2}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{3}}{\rm{.}}}&{{\rm{1}}{\rm{.0}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\end{array}\)
The rate equation for the above data is

320513 For the decomposition of HI at \(1000 \mathrm{~K}\), the following data were obtained

[HI] M Rate of decomposition of HI (mole \(L^{-1} \mathrm{~s}^{-1}\) )

\(0.1 \quad 2.75 \times 10^{-8}\)

\(0.2 \quad 11 \times 10^{-8}\)

\(0.3 \quad 24.75 \times 10^{-8}\)

The order of reaction is:

320514 At \(518^{\circ} \mathrm{C}\), the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 Torr \({{\text{s}}^{{\text{ - 1}}}}\) when 5% had reacted and 0.5 torr \({{\text{s}}^{{\text{ - 1}}}}\) when 33% had reacted. The order of the reaction is :

320510 What is the order of a chemical reaction \({\rm{A + 2B}}\mathop \to \limits^k {\rm{C}}\), if the rate of formation of C increases by a factor of 2.82 on doubling the concentration of A and increases by a factor of 9 on tripling the concentration of B ?

320511 If \(50 \%\) of a reaction occurs in 100 seconds and \(75 \%\) of the reaction occurs in 200 seconds, the order of this reaction is:

320512 The experimental data for the reaction,
\({\rm{2A + }}{{\rm{B}}_{\rm{2}}} \to {\rm{2AB,}}\,\,{\rm{is }}\)
\(\begin{array}{*{20}{c}}\begin{array}{l}{\rm{Expt}}\\\,\,{\rm{No}}{\rm{.}}\end{array}&{\left[ {\rm{A}} \right]}&{\left[ {{{\rm{B}}_{\rm{2}}}} \right]}&{{\rm{Rate}}\,\,{\rm{(}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}}\\{{\rm{1}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{2}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{3}}{\rm{.}}}&{{\rm{1}}{\rm{.0}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\end{array}\)
The rate equation for the above data is

320513 For the decomposition of HI at \(1000 \mathrm{~K}\), the following data were obtained

[HI] M Rate of decomposition of HI (mole \(L^{-1} \mathrm{~s}^{-1}\) )

\(0.1 \quad 2.75 \times 10^{-8}\)

\(0.2 \quad 11 \times 10^{-8}\)

\(0.3 \quad 24.75 \times 10^{-8}\)

The order of reaction is:

320514 At \(518^{\circ} \mathrm{C}\), the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 Torr \({{\text{s}}^{{\text{ - 1}}}}\) when 5% had reacted and 0.5 torr \({{\text{s}}^{{\text{ - 1}}}}\) when 33% had reacted. The order of the reaction is :

320510 What is the order of a chemical reaction \({\rm{A + 2B}}\mathop \to \limits^k {\rm{C}}\), if the rate of formation of C increases by a factor of 2.82 on doubling the concentration of A and increases by a factor of 9 on tripling the concentration of B ?

320511 If \(50 \%\) of a reaction occurs in 100 seconds and \(75 \%\) of the reaction occurs in 200 seconds, the order of this reaction is:

320512 The experimental data for the reaction,
\({\rm{2A + }}{{\rm{B}}_{\rm{2}}} \to {\rm{2AB,}}\,\,{\rm{is }}\)
\(\begin{array}{*{20}{c}}\begin{array}{l}{\rm{Expt}}\\\,\,{\rm{No}}{\rm{.}}\end{array}&{\left[ {\rm{A}} \right]}&{\left[ {{{\rm{B}}_{\rm{2}}}} \right]}&{{\rm{Rate}}\,\,{\rm{(}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}}\\{{\rm{1}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{2}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{3}}{\rm{.}}}&{{\rm{1}}{\rm{.0}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\end{array}\)
The rate equation for the above data is

320513 For the decomposition of HI at \(1000 \mathrm{~K}\), the following data were obtained

[HI] M Rate of decomposition of HI (mole \(L^{-1} \mathrm{~s}^{-1}\) )

\(0.1 \quad 2.75 \times 10^{-8}\)

\(0.2 \quad 11 \times 10^{-8}\)

\(0.3 \quad 24.75 \times 10^{-8}\)

The order of reaction is:

320514 At \(518^{\circ} \mathrm{C}\), the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 Torr \({{\text{s}}^{{\text{ - 1}}}}\) when 5% had reacted and 0.5 torr \({{\text{s}}^{{\text{ - 1}}}}\) when 33% had reacted. The order of the reaction is :

320510 What is the order of a chemical reaction \({\rm{A + 2B}}\mathop \to \limits^k {\rm{C}}\), if the rate of formation of C increases by a factor of 2.82 on doubling the concentration of A and increases by a factor of 9 on tripling the concentration of B ?

320511 If \(50 \%\) of a reaction occurs in 100 seconds and \(75 \%\) of the reaction occurs in 200 seconds, the order of this reaction is:

320512 The experimental data for the reaction,
\({\rm{2A + }}{{\rm{B}}_{\rm{2}}} \to {\rm{2AB,}}\,\,{\rm{is }}\)
\(\begin{array}{*{20}{c}}\begin{array}{l}{\rm{Expt}}\\\,\,{\rm{No}}{\rm{.}}\end{array}&{\left[ {\rm{A}} \right]}&{\left[ {{{\rm{B}}_{\rm{2}}}} \right]}&{{\rm{Rate}}\,\,{\rm{(}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}}\\{{\rm{1}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{2}}{\rm{.}}}&{{\rm{0}}{\rm{.50}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\\{{\rm{3}}{\rm{.}}}&{{\rm{1}}{\rm{.0}}}&{{\rm{1}}{\rm{.00}}}&{{\rm{3}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}}\end{array}\)
The rate equation for the above data is

320513 For the decomposition of HI at \(1000 \mathrm{~K}\), the following data were obtained

[HI] M Rate of decomposition of HI (mole \(L^{-1} \mathrm{~s}^{-1}\) )

\(0.1 \quad 2.75 \times 10^{-8}\)

\(0.2 \quad 11 \times 10^{-8}\)

\(0.3 \quad 24.75 \times 10^{-8}\)

The order of reaction is:

320514 At \(518^{\circ} \mathrm{C}\), the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 Torr \({{\text{s}}^{{\text{ - 1}}}}\) when 5% had reacted and 0.5 torr \({{\text{s}}^{{\text{ - 1}}}}\) when 33% had reacted. The order of the reaction is :