164244
For the reaction \(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) rate \& rate constant are \(1.02 \times 10^{-4}\) and \(3.4 \times 10^{-5} \mathrm{sec}^{-1}\) respectively then concentration of \(\mathrm{N}_2 \mathrm{O}_5\) at that time will be :
1 1.732
2 3.0
3 2.25
4 4.15
Explanation:
\(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) is example of zero order reaction hence \( r=k\left \) \( 1.02 \times 10^{-4}=3.4 \times 10^{-5}\left \) \( {\left=\frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}}=3.0} \)
NCERT-XII-73
7 RBTS PAPER
164246
If temperature is increased by \(30^{\circ} \mathrm{C}\) the rate is nearly increased by :
1 Doubled
2 Tripled
3 Six times
4 Eight times
Explanation:
For every \(10^{\circ}\) rise in temperature rate is nearly doubled so for \(30^{\circ} \mathrm{C}\) rate increased to \((2)^3=8\) times.
NCERT-XII-78
7 RBTS PAPER
164247
What determines the criteria for an effective collision :
1 Activation energy
2 Proper orientation of molecules
3 Both
4 None
Explanation:
In collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision.
NCERT-XII-83
7 RBTS PAPER
164248
The activation energy for an endothermic chemical reaction \(A \rightarrow B\) is \(E_a\) in forward direction. The activation energy for a reverse reaction :
1 is negative \(E_a\)
2 can be less than or more than \(\mathrm{E}_a\)
3 Always more than \(\mathrm{E}_{\mathrm{a}}\)
4 Always less than \(\mathrm{E}_a\)
Explanation:
Endothermic graph \(X\) is always less than \(E_a\).
NCERT-XII-79
7 RBTS PAPER
164249
For a reaction, activation energy \(E_a=1915 \mathrm{~J}\). The rate constant at \(200 \mathrm{~K}\) is \(1.6 \times 10^6 \mathrm{~s}^{-1}\). The rate constant is \(3.2 \times 10^6 \mathrm{~s}^{-1}\). The final temperature is :
164244
For the reaction \(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) rate \& rate constant are \(1.02 \times 10^{-4}\) and \(3.4 \times 10^{-5} \mathrm{sec}^{-1}\) respectively then concentration of \(\mathrm{N}_2 \mathrm{O}_5\) at that time will be :
1 1.732
2 3.0
3 2.25
4 4.15
Explanation:
\(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) is example of zero order reaction hence \( r=k\left \) \( 1.02 \times 10^{-4}=3.4 \times 10^{-5}\left \) \( {\left=\frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}}=3.0} \)
NCERT-XII-73
7 RBTS PAPER
164246
If temperature is increased by \(30^{\circ} \mathrm{C}\) the rate is nearly increased by :
1 Doubled
2 Tripled
3 Six times
4 Eight times
Explanation:
For every \(10^{\circ}\) rise in temperature rate is nearly doubled so for \(30^{\circ} \mathrm{C}\) rate increased to \((2)^3=8\) times.
NCERT-XII-78
7 RBTS PAPER
164247
What determines the criteria for an effective collision :
1 Activation energy
2 Proper orientation of molecules
3 Both
4 None
Explanation:
In collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision.
NCERT-XII-83
7 RBTS PAPER
164248
The activation energy for an endothermic chemical reaction \(A \rightarrow B\) is \(E_a\) in forward direction. The activation energy for a reverse reaction :
1 is negative \(E_a\)
2 can be less than or more than \(\mathrm{E}_a\)
3 Always more than \(\mathrm{E}_{\mathrm{a}}\)
4 Always less than \(\mathrm{E}_a\)
Explanation:
Endothermic graph \(X\) is always less than \(E_a\).
NCERT-XII-79
7 RBTS PAPER
164249
For a reaction, activation energy \(E_a=1915 \mathrm{~J}\). The rate constant at \(200 \mathrm{~K}\) is \(1.6 \times 10^6 \mathrm{~s}^{-1}\). The rate constant is \(3.2 \times 10^6 \mathrm{~s}^{-1}\). The final temperature is :
164244
For the reaction \(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) rate \& rate constant are \(1.02 \times 10^{-4}\) and \(3.4 \times 10^{-5} \mathrm{sec}^{-1}\) respectively then concentration of \(\mathrm{N}_2 \mathrm{O}_5\) at that time will be :
1 1.732
2 3.0
3 2.25
4 4.15
Explanation:
\(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) is example of zero order reaction hence \( r=k\left \) \( 1.02 \times 10^{-4}=3.4 \times 10^{-5}\left \) \( {\left=\frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}}=3.0} \)
NCERT-XII-73
7 RBTS PAPER
164246
If temperature is increased by \(30^{\circ} \mathrm{C}\) the rate is nearly increased by :
1 Doubled
2 Tripled
3 Six times
4 Eight times
Explanation:
For every \(10^{\circ}\) rise in temperature rate is nearly doubled so for \(30^{\circ} \mathrm{C}\) rate increased to \((2)^3=8\) times.
NCERT-XII-78
7 RBTS PAPER
164247
What determines the criteria for an effective collision :
1 Activation energy
2 Proper orientation of molecules
3 Both
4 None
Explanation:
In collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision.
NCERT-XII-83
7 RBTS PAPER
164248
The activation energy for an endothermic chemical reaction \(A \rightarrow B\) is \(E_a\) in forward direction. The activation energy for a reverse reaction :
1 is negative \(E_a\)
2 can be less than or more than \(\mathrm{E}_a\)
3 Always more than \(\mathrm{E}_{\mathrm{a}}\)
4 Always less than \(\mathrm{E}_a\)
Explanation:
Endothermic graph \(X\) is always less than \(E_a\).
NCERT-XII-79
7 RBTS PAPER
164249
For a reaction, activation energy \(E_a=1915 \mathrm{~J}\). The rate constant at \(200 \mathrm{~K}\) is \(1.6 \times 10^6 \mathrm{~s}^{-1}\). The rate constant is \(3.2 \times 10^6 \mathrm{~s}^{-1}\). The final temperature is :
NEET Test Series from KOTA - 10 Papers In MS WORD
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7 RBTS PAPER
164244
For the reaction \(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) rate \& rate constant are \(1.02 \times 10^{-4}\) and \(3.4 \times 10^{-5} \mathrm{sec}^{-1}\) respectively then concentration of \(\mathrm{N}_2 \mathrm{O}_5\) at that time will be :
1 1.732
2 3.0
3 2.25
4 4.15
Explanation:
\(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) is example of zero order reaction hence \( r=k\left \) \( 1.02 \times 10^{-4}=3.4 \times 10^{-5}\left \) \( {\left=\frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}}=3.0} \)
NCERT-XII-73
7 RBTS PAPER
164246
If temperature is increased by \(30^{\circ} \mathrm{C}\) the rate is nearly increased by :
1 Doubled
2 Tripled
3 Six times
4 Eight times
Explanation:
For every \(10^{\circ}\) rise in temperature rate is nearly doubled so for \(30^{\circ} \mathrm{C}\) rate increased to \((2)^3=8\) times.
NCERT-XII-78
7 RBTS PAPER
164247
What determines the criteria for an effective collision :
1 Activation energy
2 Proper orientation of molecules
3 Both
4 None
Explanation:
In collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision.
NCERT-XII-83
7 RBTS PAPER
164248
The activation energy for an endothermic chemical reaction \(A \rightarrow B\) is \(E_a\) in forward direction. The activation energy for a reverse reaction :
1 is negative \(E_a\)
2 can be less than or more than \(\mathrm{E}_a\)
3 Always more than \(\mathrm{E}_{\mathrm{a}}\)
4 Always less than \(\mathrm{E}_a\)
Explanation:
Endothermic graph \(X\) is always less than \(E_a\).
NCERT-XII-79
7 RBTS PAPER
164249
For a reaction, activation energy \(E_a=1915 \mathrm{~J}\). The rate constant at \(200 \mathrm{~K}\) is \(1.6 \times 10^6 \mathrm{~s}^{-1}\). The rate constant is \(3.2 \times 10^6 \mathrm{~s}^{-1}\). The final temperature is :
164244
For the reaction \(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) rate \& rate constant are \(1.02 \times 10^{-4}\) and \(3.4 \times 10^{-5} \mathrm{sec}^{-1}\) respectively then concentration of \(\mathrm{N}_2 \mathrm{O}_5\) at that time will be :
1 1.732
2 3.0
3 2.25
4 4.15
Explanation:
\(2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2\) is example of zero order reaction hence \( r=k\left \) \( 1.02 \times 10^{-4}=3.4 \times 10^{-5}\left \) \( {\left=\frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}}=3.0} \)
NCERT-XII-73
7 RBTS PAPER
164246
If temperature is increased by \(30^{\circ} \mathrm{C}\) the rate is nearly increased by :
1 Doubled
2 Tripled
3 Six times
4 Eight times
Explanation:
For every \(10^{\circ}\) rise in temperature rate is nearly doubled so for \(30^{\circ} \mathrm{C}\) rate increased to \((2)^3=8\) times.
NCERT-XII-78
7 RBTS PAPER
164247
What determines the criteria for an effective collision :
1 Activation energy
2 Proper orientation of molecules
3 Both
4 None
Explanation:
In collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision.
NCERT-XII-83
7 RBTS PAPER
164248
The activation energy for an endothermic chemical reaction \(A \rightarrow B\) is \(E_a\) in forward direction. The activation energy for a reverse reaction :
1 is negative \(E_a\)
2 can be less than or more than \(\mathrm{E}_a\)
3 Always more than \(\mathrm{E}_{\mathrm{a}}\)
4 Always less than \(\mathrm{E}_a\)
Explanation:
Endothermic graph \(X\) is always less than \(E_a\).
NCERT-XII-79
7 RBTS PAPER
164249
For a reaction, activation energy \(E_a=1915 \mathrm{~J}\). The rate constant at \(200 \mathrm{~K}\) is \(1.6 \times 10^6 \mathrm{~s}^{-1}\). The rate constant is \(3.2 \times 10^6 \mathrm{~s}^{-1}\). The final temperature is :
