Help with Chemistry Kinetics: Half-Life Calculation

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SUMMARY

The discussion focuses on calculating the half-life of the decomposition reaction of compound AB, given initial rate data. The initial concentrations of AB are 0.200 M, 0.400 M, and 0.600 M, with corresponding initial rates of 3.20 x 10^-3 mol/L*s, 1.28 x 10^-2 mol/L*s, and 2.88 x 10^-2 mol/L*s. To determine the half-life for an initial concentration of 1.00 M AB, one must first establish the order of the reaction based on the relationship between concentration and initial rate. This analysis will lead to the calculation of the half-life using the appropriate rate law.

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marcuss
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Need Help!-Chemistry kinetics

1. Consider the following initial rate data for the decomposition of compound AB to give A and B:
[AB]o(mol/L) Initial Rate(mol/L*s)
.200 3.20*10^-3
.400 1.28*10^-2
.600 2.88*10^-2

2. Determine the half-life for the decomposition reaction initially having 1.00M AB present.

3. If someone could just give me a clue what to do i would really appreciate it, thank you
 
Last edited:
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How does the initial rate depend on the concentration? What is the order of the reaction?
 

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