164250
A. Rate constant determinaed from Arrhenius equation are fairly accurate for simple as well as complex molecules. B. Reactant molecules undergo chemical change irrespective of their orientation during collison.
1 A and B both correct
2 A and B both incorrect
3 A correct and B incorrect
4 A incorrect and B correct
Explanation:
NCERT-XII-79
7 RBTS PAPER
164251
For a reaction \(A+B \rightarrow C\), the experimental rate law is found to be \(R=R[A]^1[B]^{1 / 2}\). Find the rate of reaction when \([A]=0.5 \mathrm{M},[B]=0.1 \mathrm{M}\) and \(K=.03\) :
164252
Correct Match : I II a. i. First order b. ii. Zero order c. d.
1 \(a \& b=i, c \& d=i i\)
2 \(a \& c=i, b \& d=i i\)
3 \(a \& d=i, b \& c=i i\)
4 \(a=i, b \& c \& d=i i\)
Explanation:
For zero order reaction \(=-k t+\left \quad-\) ve slope \(\frac{-\left}{t}=-K \quad\) No slope or first order reaction \(\frac{\mathrm{dx}}{\mathrm{dt}} \propto\) [Concentration \(^{-1}\) \( \log =\left(\frac{-K}{2.303}\right) t+\log \left \)Slope-ve
NCERT-XII-78
7 RBTS PAPER
164253
For a gaseous reaction following data is given : \( A \rightarrow \text { B K }_1=10^{15} e^{-2000 / T} \) \( C \rightarrow D_2=10^{14} e^{-1000 / T} \) The temperature at which \(K_1=K_2\) is :
164250
A. Rate constant determinaed from Arrhenius equation are fairly accurate for simple as well as complex molecules. B. Reactant molecules undergo chemical change irrespective of their orientation during collison.
1 A and B both correct
2 A and B both incorrect
3 A correct and B incorrect
4 A incorrect and B correct
Explanation:
NCERT-XII-79
7 RBTS PAPER
164251
For a reaction \(A+B \rightarrow C\), the experimental rate law is found to be \(R=R[A]^1[B]^{1 / 2}\). Find the rate of reaction when \([A]=0.5 \mathrm{M},[B]=0.1 \mathrm{M}\) and \(K=.03\) :
164252
Correct Match : I II a. i. First order b. ii. Zero order c. d.
1 \(a \& b=i, c \& d=i i\)
2 \(a \& c=i, b \& d=i i\)
3 \(a \& d=i, b \& c=i i\)
4 \(a=i, b \& c \& d=i i\)
Explanation:
For zero order reaction \(=-k t+\left \quad-\) ve slope \(\frac{-\left}{t}=-K \quad\) No slope or first order reaction \(\frac{\mathrm{dx}}{\mathrm{dt}} \propto\) [Concentration \(^{-1}\) \( \log =\left(\frac{-K}{2.303}\right) t+\log \left \)Slope-ve
NCERT-XII-78
7 RBTS PAPER
164253
For a gaseous reaction following data is given : \( A \rightarrow \text { B K }_1=10^{15} e^{-2000 / T} \) \( C \rightarrow D_2=10^{14} e^{-1000 / T} \) The temperature at which \(K_1=K_2\) is :
164250
A. Rate constant determinaed from Arrhenius equation are fairly accurate for simple as well as complex molecules. B. Reactant molecules undergo chemical change irrespective of their orientation during collison.
1 A and B both correct
2 A and B both incorrect
3 A correct and B incorrect
4 A incorrect and B correct
Explanation:
NCERT-XII-79
7 RBTS PAPER
164251
For a reaction \(A+B \rightarrow C\), the experimental rate law is found to be \(R=R[A]^1[B]^{1 / 2}\). Find the rate of reaction when \([A]=0.5 \mathrm{M},[B]=0.1 \mathrm{M}\) and \(K=.03\) :
164252
Correct Match : I II a. i. First order b. ii. Zero order c. d.
1 \(a \& b=i, c \& d=i i\)
2 \(a \& c=i, b \& d=i i\)
3 \(a \& d=i, b \& c=i i\)
4 \(a=i, b \& c \& d=i i\)
Explanation:
For zero order reaction \(=-k t+\left \quad-\) ve slope \(\frac{-\left}{t}=-K \quad\) No slope or first order reaction \(\frac{\mathrm{dx}}{\mathrm{dt}} \propto\) [Concentration \(^{-1}\) \( \log =\left(\frac{-K}{2.303}\right) t+\log \left \)Slope-ve
NCERT-XII-78
7 RBTS PAPER
164253
For a gaseous reaction following data is given : \( A \rightarrow \text { B K }_1=10^{15} e^{-2000 / T} \) \( C \rightarrow D_2=10^{14} e^{-1000 / T} \) The temperature at which \(K_1=K_2\) is :
164250
A. Rate constant determinaed from Arrhenius equation are fairly accurate for simple as well as complex molecules. B. Reactant molecules undergo chemical change irrespective of their orientation during collison.
1 A and B both correct
2 A and B both incorrect
3 A correct and B incorrect
4 A incorrect and B correct
Explanation:
NCERT-XII-79
7 RBTS PAPER
164251
For a reaction \(A+B \rightarrow C\), the experimental rate law is found to be \(R=R[A]^1[B]^{1 / 2}\). Find the rate of reaction when \([A]=0.5 \mathrm{M},[B]=0.1 \mathrm{M}\) and \(K=.03\) :
164252
Correct Match : I II a. i. First order b. ii. Zero order c. d.
1 \(a \& b=i, c \& d=i i\)
2 \(a \& c=i, b \& d=i i\)
3 \(a \& d=i, b \& c=i i\)
4 \(a=i, b \& c \& d=i i\)
Explanation:
For zero order reaction \(=-k t+\left \quad-\) ve slope \(\frac{-\left}{t}=-K \quad\) No slope or first order reaction \(\frac{\mathrm{dx}}{\mathrm{dt}} \propto\) [Concentration \(^{-1}\) \( \log =\left(\frac{-K}{2.303}\right) t+\log \left \)Slope-ve
NCERT-XII-78
7 RBTS PAPER
164253
For a gaseous reaction following data is given : \( A \rightarrow \text { B K }_1=10^{15} e^{-2000 / T} \) \( C \rightarrow D_2=10^{14} e^{-1000 / T} \) The temperature at which \(K_1=K_2\) is :
