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For second order reaction, the initial concentration of reactant A is 0.24 M. If the rate constant is 8.1 x 10-2 M-1 s-1, what is the concentration of A after 29 seconds?
Given the following balanced equation :
2NO(g) + Cl2(g) → 2NOCl(g)
If the rate of disappearance of Cl2 is 4.84 x 10-2 Ms-1, what is the rate of disappearance of NO?
1.45 x 10-2 Ms-1
2.42 x 10-2 Ms-1
3.67 x 10-2 Ms-1
9.68 x 10-2 Ms-1
In the chemical reaction, the successful formation of products depends on the following factors EXCEPT:
The collisions between reacting molecules must be effective
The colliding molecules must approach each other in the right orientation
The energy of colliding molecules must be equal to or more than activation energy
A collision between molecules must produce sufficient energy to overcome the activation energy
Choose the correct statement regarding the changes occur to the activation energy (Ea), rate constant (k) and percentage yield when a catalyst is added to a chemical reaction.
lower activation energy, k unchanged and % yield increased
lower activation energy, k unchanged and % yield unchanged
higher activation energy, k decreased and % yield increased
higher activation energy, k unchanged and % yield unchanged
The reaction A + 2B → products was found to have the rate law, k = k[A][B]2. Predict by what factor the rate of reaction will increase when the concentration of B is doubled and the concentration of A remained uncanged
The overall order for the reaction,
2A + B → C
is one and with respect to B the order is zero. Which of the following statements is true?
The rate law of the reaction is rate =k[A]2[B]
The formation of C is double the appearance of A
The rate of reaction would increase with increasing concentration B
The half-life of the reaction is independent on the concentration of the reactants
The catalyst alters the rate of a chemical reaction by,
providing an alternative pathway with a lower Ea
changing the products formed in the direction of the reaction
providing a surface on which the molecules react
increasing the frequencies of collisions between molecules
The first order rate constant for the decomposition of 0.5 M compound A at 100oC is 0.03 min-1. Calculate the half-life of A.
The rate constant for a second order reaction at 30oC is 2.0 x 10-6 M-1s-1. The activation energy for this is 108 kJ mol-1. By using Arrhenius equation, determine the collision frequency factor, A for the reaction.
5.0 x 1012
6.0 x 1012
8.0 x 1012
1.0 x 1013
Which of the following statements about catalyst is true?
It does not take part in the reaction
It increase the yield of the reaction
It provides an alternative mechanism for the reaction
It increases the number of collisions between reacting molecules per second