Govt Exams
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
Overall order = sum of exponents in rate law = 1 + 2 = 3 (third order reaction)
The rate-determining step (slowest step) controls the overall reaction rate, regardless of how many fast equilibrium steps precede it
For zero-order reaction: [A]₀ - [A]ₜ = kt. So 0.5 - 0.1 = 0.02 × t, giving t = 20 s
The exponent of [NO] in the rate law is 2, making the reaction second order with respect to NO
According to collision theory, collisions must have both proper spatial orientation and energy ≥ activation energy to result in a reaction.