The rate law is an equation that relates the reaction rate with concentrations or pressures of reactants and constant parameters.
Rate Equation: This is the mathematical representation of a rate law, showing the relationship between reaction rate and concentration of reactants. It’s like specific instructions in our cookie recipe – e.g., “Mix 2 cups flour with 1 cup sugar”.
Rate-Determining Step: In multi-step reactions, this is slowest step that determines overall reaction speed. It’s like waiting for dough to chill in fridge – no matter how fast we mix ingredients, we can’t proceed until dough has chilled.
Integrated Rate Law: This formulates relation between concentration of reactants and time; it helps predict amounts at any given point during reaction. It’s like knowing exactly when our cookies will be perfectly baked based on oven temperature and initial dough amount.
AP Chemistry - 5.2 Introduction to Rate Law
AP Chemistry - 5.3 Concentration Changes Over Time
AP Chemistry - 5.4 Elementary Reactions
AP Chemistry - 5.8 Reaction Mechanism and Rate Law
A reaction has a rate law of R = k [A][B]. With respect to A, what is the order of reaction?
A reaction has a rate law of the following: R = k [A][B]. What is the overall order of reaction?
The rate law for the following reaction is R = k[XY]^2. The initial rate of the reaction was found to be 0.16 mol/Ls when the initial concentration of XY is 0.40 mol/L. What is the value of the rate constant, k?
The rate law for the following reaction is R = k[A]^2. The initial rate of the reaction is defined as 0.080 mol/Ls, whereas the initial concentration of X is 0.20 mol/L. What is the value of the rate constant, k, for this reaction?
The following mechanism is executed: (Step 1: H2O2 + I^- → IO^- + H2O) (Step 2: H2O2 + IO^- → H2O + O2 + I^-). Which statement is true about the overall reaction and rate law?
The reaction described [O3(g) + O(g) → 2O2(g)] is the decomposition of O3. With an addition of NO, the reaction proceeds in two elementary steps and a mechanism is shown: [Step 1: O3 + NO → NO2 + O2 (slow)] [Step 2: NO2 + O → NO + O2 (fast)]. Which is the rate law?
A mechanism is shown: [Step 1: 2NO2(g) → NO3(g) + NO(g) (slow)] [Step 2: NO3(g) + CO(g) → NO2(g) + CO2(g) (fast)]. Which is the correct rate law?
What is the rate law for the following reaction: 2NO2(g) → NO(g) + NO3(g)
What is the type of elementary step and rate law for A + 2B → C?
Rate law is used to figure out ________________________.
The entire rate law is based on which of the following?
In most cases, the rate-determining step rate law isn't the rate law for the entire equation. Which of the following is an exception?
A mechanism is shown below: [Step 2: 2X(g) ⇄ X2(g) (fast)] [X2(g) + Y(g) → X2Y(g) (slow)] The rate law is consistent with the one of the hypothetical reaction 2X(g) + Y(g) → X2Y(g). Which of the following is consistent with this mechanism?
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