Govt Exams
Rate constant k is independent of reactant concentration; it depends on T, nature of reactants, and catalyst
The slowest step in a mechanism is the rate-determining step (RDS), which is step 2
0 = 0.5 - 0.02t; t = 0.5/0.02 = 25 s
Not all collisions are effective; only those with proper orientation and sufficient energy lead to reaction
After 90 min = 3 half-lives, remaining = (1/2)³ = 1/8
Overall order = sum of exponents in rate law = 2 + 1 = 3 (third order)
For elementary reactions, the rate law is determined by the stoichiometry: Rate = k[A]²[B], as 2 A molecules and 1 B molecule participate
A straight line in [A] vs time plot indicates [A] = [A]₀ - kt, which is the integrated rate law for zero-order reactions
Since the reaction is first-order in B and zero-order in A, Rate ∝ [B]. Increasing [B] by 4 times increases Rate by 4 times
A catalyst works by providing an alternative mechanism with lower Ea, thus increasing reaction rate without being consumed