1
JEE Main 2019 (Online) 8th April Evening Slot
+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
$$({k_1} - {k_2})[A]$$
2
JEE Main 2019 (Online) 8th April Morning Slot
+4
-1
If solublity product of Zr3(PO4)4 is denoted by Ksp and its molar solubility is denoted by S, then which of the following relation between S and Ksp is correct ?
A
$$S = {\left( {{{{K_{sp}}} \over {929}}} \right)^{1/9}}$$
B
$$S = {\left( {{{{K_{sp}}} \over {6912}}} \right)^{1/7}}$$
C
$$S = {\left( {{{{K_{sp}}} \over {144}}} \right)^{1/6}}$$
D
$$S = {\left( {{{{K_{sp}}} \over {216}}} \right)^{1/7}}$$
3
JEE Main 2019 (Online) 8th April Morning Slot
+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 :

[A] (mol L-1) [B] (mol L-1) Initial Rate (mol L-1s-1)
0.05 0.05 0.045
0.10 0.05 0.090
0.20 0.10 0.72
A
Rate = k[A][B]2
B
Rate = k[A]2[B]2
C
Rate = k[A]2[B]
D
Rate = k[A][B]
4
JEE Main 2019 (Online) 12th January Evening Slot
+4
-1
For a reaction consider the plot of $$\ell$$n k versus 1/T given in the figure. If the rate constant of this reaction at 400 K is 10–5 s–1, then the rate constant at 500 K is –

A
10$$-$$4 s$$-$$1
B
4 $$\times$$ 10$$-$$4 s$$-$$1
C
10$$-$$6 s$$-$$1
D
2 $$\times$$ 10$$-$$4 s$$-$$1
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