1
JEE Main 2016 (Online) 10th April Morning Slot
MCQ (Single Correct Answer)
+4
-1
Change Language
The rate law for the reaction below is given by the expression k [A] [B]

A + B $$ \to $$ Product

If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be :
A
k
B
k/3
C
3k
D
9k
2
JEE Main 2016 (Online) 9th April Morning Slot
MCQ (Single Correct Answer)
+4
-1
Change Language
The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below :

O3(g) + Cl$${^ \bullet }$$ (g) $$ \to $$ O2(g) + ClO$${^ \bullet }$$ (g) . . . . . .(i)

ki = 5.2 × 109 L mol−1 s−1

ClO$${^ \bullet }$$(g) + O$${^ \bullet }$$(g) $$ \to $$ O2(g) + Cl$${^ \bullet }$$ (g) . . . . . . (ii)

kii = 2.6 × 1010 L mol−1 s−1

The closest rate constant for the overall reaction O3(g) + O$${^ \bullet }$$ (g) $$ \to $$ 2 O2(g) is :
A
5.2 × 109 L mol−1 s−1
B
2.6 × 1010 L mol−1 s−1
C
3.1 × 1010 L mol−1 s−1
D
1.4 × 1020 L mol−1 s−1
3
JEE Main 2016 (Offline)
MCQ (Single Correct Answer)
+4
-1
Change Language
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
4
JEE Main 2015 (Offline)
MCQ (Single Correct Answer)
+4
-1
Change Language
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
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