For each of the scenarios, identify the order with respect to the reactant, A. A⟶products The half‑life of A is independent of the initial concentration of [A].   A three‑fold increase in the initial concentration of A leads to a nine‑fold increase in the initial rate.   A three‑fold increase in the initial concentration of A leads to a 1.73‑fold increase in the initial rate.   The time required for [A] to decrease from [A]0 to [A]0/2 is equal to the time required for [A] to decrease from [A]0/2 to [A]0/4.   The rate of decrease of [A] is a constant.

Consider the mechanism. Step 1: А +В — С slow Step 2: А +С — D fast Overall: 2 A + B → D -> Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =

PART A The rate of the reaction in terms of the "disappearance of reactant" includes the change in the concentration of the reactant, the time interval, and the coefficient of the reactant. Consider the following reaction: 2A+3B→3C+2D2A+3B→3C+2D The concentrations of reactant A at three different time intervals are given. Use the following data to determine the average rate of reaction in terms of the disappearance of reactant AA between time = 0 ss  and time = 20 ss. Time (ss) 0 20 40 [A](M)[A](�) 0.0800 0.0480 0.0360 Express your answer in molar concentration per second to three significant figures. PART B

Find the half life time of the following reaction :  A---> C Rate law = 1.0s^-1 *[A]

The rate of the given reaction is 0.240 M/s. A+ 4B 2C What is the relative rate of change of each species in the reaction? Δ[Α] ΔΙ Δ[Β] A[C] ΔΙ = 11 ||

Given the following rate law, what is the order of the reaction for each item?

Please help me i have no clue what I'm doing.   A reaction is found to be second order with a rate constant of 3.45×10^-5 M^-1s^-1. The reaction began with 4.354 reactant. How much reactant remains (in M) after 1 hour?