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marta [7]
3 years ago
14

The volume of 5.00 M KBr needed to have 1.00 mol KBr mL

Chemistry
1 answer:
astra-53 [7]3 years ago
7 0

Answer: molarity = mole solute/ liter of solution.

=> volume= mole/molarity = 1/5 = 0.2 L = 200mL

Explanation:

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What is the half-life of a first-order reaction if it takes 4.4 x 102 seconds for the concentration to decrease from 0.50 M to 0
elena55 [62]

Answer: The half-life of a first-order reaction is, 3.3\times 10^2s

Explanation:

All the radioactive reactions follows first order kinetics.

Rate law expression for first order kinetics is given by the equation:

k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}

where,  

k = rate constant = ?

t = time taken = 440 s

[A_o] = initial amount of the reactant = 0.50 M

[A] = left amount =  0.20 M

Putting values in above equation, we get:

k=\frac{2.303}{440s}\log\frac{0.50}{0.20}

k=2.083\times 10^{-3}s^{-1}

The equation used to calculate half life for first order kinetics:

t_{1/2}=\frac{0.693}{k}

Putting values in this equation, we get:

t_{1/2}=\frac{0.693}{2.083\times 10^{-3}s^{-1}}=332.69s=3.3\times 10^2s

Therefore, the half-life of a first-order reaction is, 3.3\times 10^2s

4 0
3 years ago
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