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2 years ago

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What is the half-life in minutes of a compound if 75.0 percent of a given sample decomposes in 40.0 minutes? Assume first-order

kinetics.

1 answer:

yaroslaw [1]2 years ago

8 0

Answer:

See below

Explanation:

.75 = 1/2^(40/h)

log .75 / ( log 1/2) = 40 / h

<u>h = half life = 96.37683 min</u>

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4 years ago

A chemist dissolves 697. mg of pure potassium hydroxide in enough water to make up 160. mL of solution. Calculate the pH of the

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$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

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3 years ago

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4 years ago

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sp2606 [1]

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