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Gnom [1K]
3 years ago
8

A chemist must dilute of aqueous aluminum chloride solution until the concentration falls to . He'll do this by adding distilled

water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
marshall27 [118]3 years ago
7 0

Answer:

0.257 L

Explanation:

The values missing in the question has been assumed with common sense so  that the concept could be applied

Initial volume of the AICI3 solution =23.1 \mathrm{mL}

Initial Molarity of the solution =833 \mathrm{mM}

Final molarity of the solution =75.0 \mathrm{mM}

Final volume of the solution =?

From Law of Dilution, M_{f} V_{f}=M_{i} V_{i}

\Rightarrow V_{f}=\frac{M_{i} V_{i}}{M_{f}}=\frac{833 \mathrm{mM} \times 23.1 \mathrm{mL}}{75.0 \mathrm{mM}}=256.564 \mathrm{mL}=0.256564 \mathrm{L}=0.257 L

Final Volume of the solution =0.257

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<u>Answer:</u> The average rate of the reaction is 7.82\times 10^{-3}M/min

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To calculate the molarity of hydrogen gas generated, we use the equation:

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Moles of hydrogen gas = 3.91\times 10^{-2}mol

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Putting values in above equation, we get:

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\text{Average rate of the reaction}=\frac{0.1564M}{20.0min}\\\\\text{Average rate of the reaction}=7.82\times 10^{-3}M/min

Hence, the average rate of the reaction is 7.82\times 10^{-3}M/min

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