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2 years ago

8

small amount wet of hydrogen gas (H2) can be prepared by the reaction of zinc with excess hydrochloric acid and trapping the gas

produced in an inverted tube initially filled with water. If the total pressure of the gas in the collection tube is 729.7 mmHg at 25°C, what is the partial pressure of the hydrogen? The vapor pressure of water is 23.8 mmHg.

1 answer:

leonid [27]2 years ago

5 0

<u>Answer:</u> The partial pressure of hydrogen is 705.9 mmHg

<u>Explanation:</u>

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the partial pressure of hydrogen gas, we use the law given by Dalton, which is:

$P_T=p_{H_2}+p_{H_2O}$

We are given:

Total pressure of the collection tube, $P_T$ = 729.8 mmHg

Vapor pressure of water, $p_{H_2O}$ = 23.8 mmHg

Putting values in above equation, we get:

$729.7=p_{H_2}+23.8\\\\p_{H_2}=729.7-23.8=705.9mmHg$

Hence, the partial pressure of hydrogen is 705.9 mmHg

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2 years ago

How many grams of water are required to produce 5.50L of hydrogen gas at 25.0 degrees C and 755mmHg?

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Answer is: 4.02 grams of water are required.
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n(H₂) = 0.993 atm · 5.5 L ÷ 0,08206 L·atm/mol·K · 298.15 K.
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3 years ago

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2 years ago

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