1
JEE Main 2017 (Offline)
+4
-1 Two reactions R1 and R2 have identical pre-exponential factors. Activation energy of R1 exceeds that of R2 by 10 kJ mol–1. If k1 and k2 are rate constants for reactions R1 and R2 respectively at 300 K, then ln(k2/k1) is equal to :
(R = 8.314 J mol–1 K–1)
A
12
B
6
C
4
D
8
2
JEE Main 2016 (Online) 10th April Morning Slot
+4
-1 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
3
JEE Main 2016 (Online) 9th April Morning Slot
+4
-1 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
4
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
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