1
JEE Main 2020 (Online) 5th September Morning Slot
+4
-1
A flask contains a mixture of compounds A and B. Both compounds decompose by first-order kinetics. The half-lives for A and B are 300 s and 180 s, respectively. If the concentrations of A and B are equal initially, the time required for the concentration of A to be four times that of B(in s) :
(Use ln 2 = 0.693)
A
180
B
120
C
300
D
900
2
JEE Main 2020 (Online) 3rd September Evening Slot
+4
-1
For the reaction
2A + 3B + $${3 \over 2}$$C $$\to$$ 3P, which statement is correct ?
A
$${{d{n_A}} \over {dt}} = {{d{n_B}} \over {dt}} = {{d{n_C}} \over {dt}}$$
B
$${{d{n_A}} \over {dt}} = {2 \over 3}{{d{n_B}} \over {dt}} = {3 \over 4}{{d{n_C}} \over {dt}}$$
C
$${{d{n_A}} \over {dt}} = {3 \over 2}{{d{n_B}} \over {dt}} = {3 \over 4}{{d{n_C}} \over {dt}}$$
D
$${{d{n_A}} \over {dt}} = {2 \over 3}{{d{n_B}} \over {dt}} = {4 \over 3}{{d{n_C}} \over {dt}}$$
3
JEE Main 2020 (Online) 3rd September Morning Slot
+4
-1
It is true that :
A
A first order reaction is always a single step reaction
B
A zero order reaction is a multistep reaction
C
A zero order reaction is a single step reaction
D
A second order reaction is always a multistep reaction
4
JEE Main 2020 (Online) 2nd September Evening Slot
+4
-1
The results given in the below table were obtained during kinetic studies of the following reaction

2A + B $$\to$$ C + D
X and Y in the given table are respectively :
A
0.3, 0.4
B
0.4, 0.3
C
0.4, 0.4
D
0.3, 0.3
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