22407.A follows first order reaction, A → product. Concentration of A, changes from 0.1 M to 0.025 M in 40 minutes. Find the rate of reaction of A when concentration of A is 0.01 M.
1.73 × 10–4 M min–1
3.47 × 10–5 M min–1
3.47 × 10–4 M min–1
1.73 × 10–5 M min–1
22408.The rate of a first order reaction is 1.5 × 10–2 mol L–1 min–1 at 0.5 M concentration of the reactant. The half life of the reaction is
23.1 min
8.73 min
7.53 min
0.383 min
22409.Radioactivity of a sample (z = 22) decreases 90% after 10 years. What will be the half–life of the sample?
5 years
2 years
3 years
10 years
22410.In a reaction, A + B → Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled, rate law for the reaction can be written as
Rate = k[A] [B]
Rate = k[A]2[B]
Rate = k[A][B]2
Rate = k[A]2[B]2
22411.Consider a reaction, aG + bH → Products. When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when the concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is:
0
1
2
3
22412.The rate equation for the reaction: 2A + B → C is found to be: rate = k [A] [B]. The correct statement in relation to this reaction is that the
units of k must be s–1
t1/2 is constant
rate of formation of C is twice the rate of disappearance of A
value of k is independent of the initial concentration of A and B.
22413.The velocity constant of a reaction at 290 K was found to be 3.2 × 10–3 S–1. When the temperature is raised to 310 K, it will be about:
9.6 × 10–3
1.28 × 10–2
6.4 × 10–3
3.2 × 10–4
22414.The rate law for a reaction between the substances A an B is given by Rate = k [A]n[B]m. On doubling the concentration of A and halving the concentration of B, the ratio of the new rate to the earlier rate of reaction will be
m + n
n – m
2(n – m)
$\dfrac{1}{2^{m+n}}$
22415.When a biochemical reaction is carried out in laboratory out side the human body in the absence of enzyme, then the rate of reaction obtained is 10–6 times, than activation energy of reaction in the presence of enzyme is:
6/RT
P is required
Different from, Ea obtained in laboratory
Can't say
22416.The rate equation for a reaction: A → B is r = K [A]°. If the initial concentration of the reactant is a mol dm–3, the half life period of the reaction is
K/a
a/K
2a/K
a/2K