7 RBTS PAPER(CHEMISTRY)
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7 RBTS PAPER

164230 For the reaction, \(2 A+B \rightarrow\) Products the following initial rates were obtained at various initial concentrations :

[A]{\([B]\)}Rate \(\left(\mathrm{mol} \mathrm{l}^{-1} \mathrm{sec}^{-1}\right)\)
\(0.1 \mathrm{M}\)\(0.2 \mathrm{M}\)0.46
\(0.2 \mathrm{M}\)\(0.2 \mathrm{M}\)1.84
\(0.2 \mathrm{M}\)\(0.1 \mathrm{M}\)0.92

The rate law for the reaction is :

1 Rate \(=k[A]^2[B]^0\)
2 Rate \(=k[A][B]\)
3 Rate \(=k[A]^2[B]\)
4 Rate \(=k[A][B]^2\)
NCERT-XII-67
7 RBTS PAPER

164231 \(\mathrm{RCOOR}^{\prime}+\mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{HCl}} \mathrm{RCOOH}+\mathrm{R}^{\prime} \mathrm{OH}\) :
What type of reaction is this :

1 \(2^{\text {nd }}\) order reaction
2 \(1^{\text {st }}\) order reaction
3 Pseudo unimolecular reaction
4 \(3^{\text {rd }}\) order reaction
NCERT-XII-78
7 RBTS PAPER

164232 The hypothetical reaction, \(A_2+B_2 \rightarrow 2 A B\) follows the following mechanism:
\( A_2 \rightleftharpoons A+A \text { (fast) } \)
\( A+B_2 \rightarrow A B+B \text { (slow) } \)
\( A+B \rightarrow A B \text { (fast) } \)
The order of the over all reaction is

1 zero
2 1
3 2
4 \(3 / 2\)
NCERT-XII-70
7 RBTS PAPER

164233 The rate of the reaction \(2 \mathrm{NO}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NOCl}\) is given by the rate equation, rate \(=k[\mathrm{NO}]^2\left[\mathrm{Cl}_2\right]\). The value of the rate constant can be increased by :

1 Increasing the temperature
2 Increasing the concentration of NO
3 Increasing the concentration of the \(\mathrm{Cl}_2\)
4 Doing all of these
NCERT-XII-67
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7 RBTS PAPER

164230 For the reaction, \(2 A+B \rightarrow\) Products the following initial rates were obtained at various initial concentrations :

[A]{\([B]\)}Rate \(\left(\mathrm{mol} \mathrm{l}^{-1} \mathrm{sec}^{-1}\right)\)
\(0.1 \mathrm{M}\)\(0.2 \mathrm{M}\)0.46
\(0.2 \mathrm{M}\)\(0.2 \mathrm{M}\)1.84
\(0.2 \mathrm{M}\)\(0.1 \mathrm{M}\)0.92

The rate law for the reaction is :

1 Rate \(=k[A]^2[B]^0\)
2 Rate \(=k[A][B]\)
3 Rate \(=k[A]^2[B]\)
4 Rate \(=k[A][B]^2\)
NCERT-XII-67
7 RBTS PAPER

164231 \(\mathrm{RCOOR}^{\prime}+\mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{HCl}} \mathrm{RCOOH}+\mathrm{R}^{\prime} \mathrm{OH}\) :
What type of reaction is this :

1 \(2^{\text {nd }}\) order reaction
2 \(1^{\text {st }}\) order reaction
3 Pseudo unimolecular reaction
4 \(3^{\text {rd }}\) order reaction
NCERT-XII-78
7 RBTS PAPER

164232 The hypothetical reaction, \(A_2+B_2 \rightarrow 2 A B\) follows the following mechanism:
\( A_2 \rightleftharpoons A+A \text { (fast) } \)
\( A+B_2 \rightarrow A B+B \text { (slow) } \)
\( A+B \rightarrow A B \text { (fast) } \)
The order of the over all reaction is

1 zero
2 1
3 2
4 \(3 / 2\)
NCERT-XII-70
7 RBTS PAPER

164233 The rate of the reaction \(2 \mathrm{NO}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NOCl}\) is given by the rate equation, rate \(=k[\mathrm{NO}]^2\left[\mathrm{Cl}_2\right]\). The value of the rate constant can be increased by :

1 Increasing the temperature
2 Increasing the concentration of NO
3 Increasing the concentration of the \(\mathrm{Cl}_2\)
4 Doing all of these
NCERT-XII-67
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7 RBTS PAPER

164230 For the reaction, \(2 A+B \rightarrow\) Products the following initial rates were obtained at various initial concentrations :

[A]{\([B]\)}Rate \(\left(\mathrm{mol} \mathrm{l}^{-1} \mathrm{sec}^{-1}\right)\)
\(0.1 \mathrm{M}\)\(0.2 \mathrm{M}\)0.46
\(0.2 \mathrm{M}\)\(0.2 \mathrm{M}\)1.84
\(0.2 \mathrm{M}\)\(0.1 \mathrm{M}\)0.92

The rate law for the reaction is :

1 Rate \(=k[A]^2[B]^0\)
2 Rate \(=k[A][B]\)
3 Rate \(=k[A]^2[B]\)
4 Rate \(=k[A][B]^2\)
NCERT-XII-67
7 RBTS PAPER

164231 \(\mathrm{RCOOR}^{\prime}+\mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{HCl}} \mathrm{RCOOH}+\mathrm{R}^{\prime} \mathrm{OH}\) :
What type of reaction is this :

1 \(2^{\text {nd }}\) order reaction
2 \(1^{\text {st }}\) order reaction
3 Pseudo unimolecular reaction
4 \(3^{\text {rd }}\) order reaction
NCERT-XII-78
7 RBTS PAPER

164232 The hypothetical reaction, \(A_2+B_2 \rightarrow 2 A B\) follows the following mechanism:
\( A_2 \rightleftharpoons A+A \text { (fast) } \)
\( A+B_2 \rightarrow A B+B \text { (slow) } \)
\( A+B \rightarrow A B \text { (fast) } \)
The order of the over all reaction is

1 zero
2 1
3 2
4 \(3 / 2\)
NCERT-XII-70
7 RBTS PAPER

164233 The rate of the reaction \(2 \mathrm{NO}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NOCl}\) is given by the rate equation, rate \(=k[\mathrm{NO}]^2\left[\mathrm{Cl}_2\right]\). The value of the rate constant can be increased by :

1 Increasing the temperature
2 Increasing the concentration of NO
3 Increasing the concentration of the \(\mathrm{Cl}_2\)
4 Doing all of these
NCERT-XII-67
For More Updates join with Us
NEET Test Series from KOTA - 10 Papers In MS WORD WhatsApp Here
7 RBTS PAPER

164230 For the reaction, \(2 A+B \rightarrow\) Products the following initial rates were obtained at various initial concentrations :

[A]{\([B]\)}Rate \(\left(\mathrm{mol} \mathrm{l}^{-1} \mathrm{sec}^{-1}\right)\)
\(0.1 \mathrm{M}\)\(0.2 \mathrm{M}\)0.46
\(0.2 \mathrm{M}\)\(0.2 \mathrm{M}\)1.84
\(0.2 \mathrm{M}\)\(0.1 \mathrm{M}\)0.92

The rate law for the reaction is :

1 Rate \(=k[A]^2[B]^0\)
2 Rate \(=k[A][B]\)
3 Rate \(=k[A]^2[B]\)
4 Rate \(=k[A][B]^2\)
NCERT-XII-67
7 RBTS PAPER

164231 \(\mathrm{RCOOR}^{\prime}+\mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{HCl}} \mathrm{RCOOH}+\mathrm{R}^{\prime} \mathrm{OH}\) :
What type of reaction is this :

1 \(2^{\text {nd }}\) order reaction
2 \(1^{\text {st }}\) order reaction
3 Pseudo unimolecular reaction
4 \(3^{\text {rd }}\) order reaction
NCERT-XII-78
7 RBTS PAPER

164232 The hypothetical reaction, \(A_2+B_2 \rightarrow 2 A B\) follows the following mechanism:
\( A_2 \rightleftharpoons A+A \text { (fast) } \)
\( A+B_2 \rightarrow A B+B \text { (slow) } \)
\( A+B \rightarrow A B \text { (fast) } \)
The order of the over all reaction is

1 zero
2 1
3 2
4 \(3 / 2\)
NCERT-XII-70
7 RBTS PAPER

164233 The rate of the reaction \(2 \mathrm{NO}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NOCl}\) is given by the rate equation, rate \(=k[\mathrm{NO}]^2\left[\mathrm{Cl}_2\right]\). The value of the rate constant can be increased by :

1 Increasing the temperature
2 Increasing the concentration of NO
3 Increasing the concentration of the \(\mathrm{Cl}_2\)
4 Doing all of these
NCERT-XII-67