1
JEE Main 2016 (Offline)
+4
-1
Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H2O2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be :
A
6.93 $$\times$$ 10-4 mol min-1
B
6.96 $$\times$$ 10-2 mol min-1
C
1.34 $$\times$$ 10-2 mol min-1
D
2.66 L min–1 at STP
2
JEE Main 2015 (Offline)
+4
-1
Higher order (>3) reactions are rare due to
A
increase in entropy and activation energy as more molecules are involved
B
shifting of equilibrium towards reactants due to elastic collisions
C
loss of active species on collision
D
low probability of simultaneous collision of all the reacting species
3
JEE Main 2014 (Offline)
+4
-1
For the non – stoichiometre reaction 2A + B $$\to$$ C + D, the following kinetic data were obtained in three separate experiments, all at 298 K.
Initial Concentration (A) Initial Concentration (B) Initial rate of formation of C (mol L-1 s-1)
0.1 M 0.1 M 1.2 x 10-3
0.1 M 0.2 M 1.2 x 10-3
0.2 M 0.1 M 2.4 x 10-3
The rate law for the formation of C is:
A
$${{dc} \over {dt}} = k[A]{[B]^2}$$
B
$${{dc} \over {dt}} = k[A]$$
C
$${{dc} \over {dt}} = k[A]{[B]}$$
D
$${{dc} \over {dt}} = k[A^2]{[B]}$$
4
JEE Main 2013 (Offline)
+4
-1
The rate of a reaction doubles when its temperature changes from 300K to 310K. Activation energy of such a reaction will be:(R = 8.314 JK–1 mol–1 and log 2 = 0.301)
A
48.6 kJ mol–1
B
58.5 kJ mol–1
C
60.5 kJ mol–1
D
53.6 kJ mol–1
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