Consider the given plot of enthalpy of the
following reaction between A and B.
A+ B $$ \to $$ C + D
Identify the incorrect statement.
A
Formation of A and B from C has highest
enthalpy of activation.
B
D is kinetically stable product.
C
C is the thermodynamically stable product
D
Activation enthalpy to form C is 5kJ mol–1
less than that to form D.
2
JEE Main 2019 (Online) 9th April Morning Slot
MCQ (Single Correct Answer)
+4
-1
The given plots represent the variation of the
concentration of a reactant R with time for two
different reactions (i) and (ii). The respective
orders of the reactions are :
A
0,1
B
1,0
C
0,2
D
1,1
3
JEE Main 2019 (Online) 8th April Evening Slot
MCQ (Single Correct Answer)
+4
-1
For a reaction scheme $$A\buildrel {{k_1}} \over
\longrightarrow B\buildrel {{k_2}} \over
\longrightarrow C$$,
if
the rate of formation of B is set to be zero then
the concentration of B is given by :
A
$${k_1}{k_2}[A]$$
B
$$\left( {{{{k_1}} \over {{k_2}}}} \right)[A]$$
C
$$({k_1} + {k_2})[A]$$
D
$$({k_1} - {k_2})[A]$$
4
JEE Main 2019 (Online) 8th April Morning Slot
MCQ (Single Correct Answer)
+4
-1
For the reaction 2A + B $$ \to $$ C, the values of initial rate at diffrent reactant concentrations are
given in the table below. The rate law for the reaction is :
