For a first order reaction the reaction rate at reactant concentration of 0.01 M is found to be 2.0 x 10-5 ,mol L-1 s-1. The half-life period of the reaction is.
220 s
30 s
300 s
347 s
For the reaction,Products, it is observed that.
Rate = k[A2[B]
Rate = k[A][B]2
Rate = k[A]2[B]2
Rate = k[A][B]
In the following reaction, how is the rate of appearance of the underlined product related to the rate of disappearance of the underlined reactant?
The reaction of hydrogen and iodine monochloride is given as.
B only
A and B both
Neither A nor B
A only
A substance 'A' decomposes by a first order reaction starting initially with [A]=2.00 m and after 200 min,[A] becomes 0.15 m.For this reaction t1/2 is.
53.49 min
50.49 min
48.45 min
46.45 min
The experimental data for the reaction
The bromination of acetone that occurs in acid solution is respresented by this equation.
