ln[A] = -kt + ln[A]₀

[A] = -kt + [A]₀

[A] = kt + [A]₀

A

B

C

D

$\frac{Δ\left[A\right]}{Δ\left[t\right]}$

$\frac{Δt}{Δ\left[A\right]}$

$\frac{Δ\left[t\right]}{ΔA}$

$\frac{Δ\left[A\right]}{Δt}$

Experimentally

The coefficients in the balanced equation

They are given

Graphing

log[A] = -kt + log[A]₀

ln[A] = -kt + ln[A]₀

[A] = -kt + [A]₀

ln[A] = kt + ln[A]₀

-50kJ

-190kJ

+190kJ

+50kJ

0kJ

Rate = k[BrO₃⁻]¹[Br⁻]¹[H₃O⁺]²

Rate = [Br⁻]¹[BrO₃⁻]¹[H₃O⁺]²

Rate = k[H₃O⁺][BrO₃⁻][Br⁻]

Rate = k[BrO₃⁻]²[Br⁻]²[H₃O⁺]¹

Rate = -k[BrO₃⁻]¹[Br⁻]¹[H₃O⁺]²

A rate law that is false

A rate law that is result of the simplification of a more complex rate law

A rate law that is incomplete, due to lacking orders

A rate law that represents the abstract concept of rate laws (Rate = k[A][B]), without specific reactants or orders

A rate law that does not have any variables calculated

The initial product and the final reactants solely

The intermediate substances of a reaction solely

The mechanism by which reactions occur; activation energy

The series of steps a reaction takes to go from reactant to product

Rate = [A]

Rate = k[A]²

Rate = k[A][B][C]

Rate = k[A][B]

Rate = [A]²[B]²

Rate = k[A₂][B]²

Rate = k[AB]ⁿ

Rate = k[A₂]ⁿ[B]ⁿ

Rate = k[AB]²

Rate = [A₂]ⁿ[B]ⁿ

Easy

Moderately easy

Moderately difficult

Difficult