2 A(g) + B(g) → C(g) + D(g) is [A]. (M) 0.150 0.450 0.450 [B]. (M) 0.300 0.300 0.150 Question 10 of 15 Rate (M/m 3.38 x 10-5 1.01 x 10-4 2.54 x 10-5 Learn More in OpenStax A) Rate = K[A] [B] B) Rate = K[A] Rate = K[A]²[B] D) Rate = K[A] [B]² Periodic Table Submit
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2 A(g) + B(g) → C(g) + D (g) is
[A]. (M)
0.150
0.450
0.450
[B]. (M)
0.300
0.300
0.150
Question 10 of 15
Rate (M/m
3.38 x 10-5
1.01 x 10-4
2.54 x 10-5
Learn More in OpenStax
A) Rate = K[A] [B]
B) Rate = K[A]
C) Rate = K[A]2[B]
D) Rate = K[A] [B]²
Periodic Table
Submit](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6543cb9f-7a09-4737-9ba8-548b67ad059a%2F570d17b8-fc59-43c6-89c2-e088fc28f1b8%2Fr8dfv0p_processed.jpeg&w=3840&q=75)
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Introduction
The rate law in chemistry is an equation used to describe the rate of a chemical reaction. It is used to calculate the rate of reaction given the concentrations of reactants and the rate constant of the reaction. The rate law equation can be written in the form:
Where "k" is the rate constant, [A] and [B] are the concentrations of the reactants, and "a" and "b" are the reaction orders for reactants A and B. The reaction order of a reactant is the power to which its concentration is raised in the rate law equation. The overall order of the reaction is the sum of the individual reaction orders.
For a single reactant, the rate law equation is simplified to:
The rate constant is determined by performing an experiment where the concentrations of the reactants are varied and the rate of the reaction is measured. From these results, a graph can be plotted to find the rate constant of the reaction.
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