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For a first order reaction A→B the reaction rate at reactant concentration of 0.01 M is found to be 2.0×10^−5 mol L^−1s^−1 . The half life period of the reaction is
02
Jun
For a first order reaction A→B the reaction rate at reactant concentration of 0.01 M is found to be 2.0×10^−5 mol L^−1s^−1 . The half life period of the reaction is For a first order reaction A→B the reaction rate at reactant concentration of 0.01 M is found to be 2.0×10^−5 mol L^−1s^−1 . The [...]
The rate of reaction between two A and B decreases by factor 4, if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is
02
Jun
The rate of reaction between two A and B decreases by factor 4, if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is The rate of reaction [...]
The thermal decomposition of HCOOH is a first-order reaction with a rate constant of 2.4×10^−3 s^−1 at certain temperature. Calculate how long will it take for three-fourths of the initial quantity of HCOOH to decompose?
02
Jun
The thermal decomposition of HCOOH is a first-order reaction with a rate constant of 2.4×10^−3 s^−1 at certain temperature. Calculate how long will it take for three-fourths of the initial quantity of HCOOH to decompose? Rate constant k varies with temperature as given by equation log k (min^−1) = 5 − 2000/T Consider the following [...]
The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. Calculate the activation energy for the reaction. [R=8.314 JK^−1 mol^−1 ]
02
Jun
The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. Calculate the activation energy for the reaction. [R=8.314 JK^−1 mol^−1 ] The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. [...]
If the rate of decomposition of N2O5 during a certain time internal is 2.4×10^−4 mol L^−1 min^−1. N2O5 →2NO2 + 2/1O2 What is the rate of formation of NO2 and O2 mol L^−1 min^−1 ?
02
Jun
If the rate of decomposition of N2O5 during a certain time internal is 2.4×10^−4 mol L^−1 min^−1. N2O5 →2NO2 + 2/1O2 What is the rate of formation of NO2 and O2 mol L^−1 min^−1 ? If the rate of decomposition of N2O5 during a certain time internal is 2.4×10^−4 mol L^−1 min^−1. N2O5 →2NO2 + [...]
In the reaction A gives product , -da/dt = k1A. If we start with 10 M of A, then after one natural life time, concentration of A is decreased to
02
Jun
In the reaction A gives product , -da/dt = k1A. If we start with 10 M of A, then after one natural life time, concentration of A is decreased to -da/dt = k1A. If we start with 10 M of A concentration of A is decreased to In the reaction A gives product then after [...]
For the reaction, 2NO + Br2 → 2NOBr following mechanism has been given: (1) NO+Br2 ⇌Fast NOBr2 (2) NOBr2 +NO gives Slow 2NOBr Hence, rate law is
02
Jun
For the reaction, 2NO + Br2 → 2NOBr following mechanism has been given: (1) NO+Br2 ⇌Fast NOBr2 (2) NOBr2 +NO gives Slow 2NOBr Hence, rate law is 2NO + Br2 → 2NOBr following mechanism has been given: (1) NO+Br2 ⇌Fast NOBr2 (2) NOBr2 +NO gives Slow 2NOBr Hence For the reaction rate law is June [...]
For nth order reaction (dx/dt)=Rate = k[A]0n Graph between log (rate) against log[A0] is of the type Lines P, Q, R, S are of the order:
02
Jun
For nth order reaction (dx/dt)=Rate = k[A]0n Graph between log (rate) against log[A0] is of the type Lines P, Q, R, S are of the order: -q For nth order reaction (dx/dt)=Rate = k[A]0n Graph between log (rate) against log[A0] is of the type Lines P R S are of the order: the activation energy [...]
Rate constant k varies with temperature as given by equation log k (min^−1) = 5 − 2000/T Consider the following about this equation
02
Jun
Rate constant k varies with temperature as given by equation log k (min^−1) = 5 − 2000/T Consider the following about this equation Rate constant k varies with temperature as given by equation log k (min^−1) = 5 − 2000/T Consider the following about this equation June 2, 2021 Category: AIIMS Last 24 Years Solved [...]
On introducing a catalyst at 300 k, the activation energy increases by 5.75 kJ/mol. The ratio of rate constant k2/k1 will be
02
Jun
On introducing a catalyst at 300 k, the activation energy increases by 5.75 kJ/mol. The ratio of rate constant k2/k1 will be On introducing a catalyst at 300 k the activation energy increases by 5.75 kJ/mol. The ratio of rate constant k2/k1 will be June 2, 2021 Category: AIIMS Last 24 Years Solved 1996 - [...]