JEE Main 2019 (Online) 10th April Evening Slot | Chemical Kinetics and Nuclear Chemistry Question 89 | Chemistry

JEE Main 2019 (Online) 10th April Evening Slot

MCQ (Single Correct Answer)

-1

For the reaction of H₂ with I₂, the rate constant is 2.5 × 10^–4 dm³ mol^–1s^–1 at 327°C and 1.0 dm³ mol^–1 at 527°C. The activation energy for the reaction, in kJ mole^–1 is : (R = 8.314 JK^–1 mol^–1 )

166

150

JEE Main 2019 (Online) 10th April Morning Slot

MCQ (Single Correct Answer)

-1

A bacterial infection in an internal wound grows as N'(t) = N₀ exp(t), where the time t is in hours. A does of antibiotic, taken orally, needs 1 hour to reach the wound. Once it reaches there, the bacterial population goes down as $${{dN} \over {dt}} = - 5{N^2}$$. What will be the plot of $${{{N_0}} \over N}$$ vs. t after 1 hour?

JEE Main 2019 (Online) 10th April Morning Slot Chemistry - Chemical Kinetics and Nuclear Chemistry Question 91 English Option 1

JEE Main 2019 (Online) 10th April Morning Slot Chemistry - Chemical Kinetics and Nuclear Chemistry Question 91 English Option 2

JEE Main 2019 (Online) 10th April Morning Slot Chemistry - Chemical Kinetics and Nuclear Chemistry Question 91 English Option 3

JEE Main 2019 (Online) 10th April Morning Slot Chemistry - Chemical Kinetics and Nuclear Chemistry Question 91 English Option 4

JEE Main 2019 (Online) 9th April Morning Slot

MCQ (Single Correct Answer)

-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 : JEE Main 2019 (Online) 9th April Morning Slot Chemistry - Chemical Kinetics and Nuclear Chemistry Question 92 English

JEE Main 2019 (Online) 9th April Morning Slot Chemistry - Chemical Kinetics and Nuclear Chemistry Question 92 English

0,1

1,0

0,2

1,1

JEE Main 2019 (Online) 8th April Evening Slot

MCQ (Single Correct Answer)

-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 :

$${k_1}{k_2}[A]$$

$$\left( {{{{k_1}} \over {{k_2}}}} \right)[A]$$

$$({k_1} + {k_2})[A]$$

$$({k_1} - {k_2})[A]$$

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