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Nuetrik [128]
2 years ago
12

A sample of oxygen gas was collected via water displacement. Since the oxygen was collected via water displacement, the sample i

s saturated with water vapor. If the total pressure of the mixture at 26.4 °C is 805 torr, what is the partial pressure of oxygen? The vapor pressure of water at 26.4 °C is 25.81 mm Hg.
Chemistry
1 answer:
lapo4ka [179]2 years ago
8 0

Answer :  The partial pressure of oxygen is, 799.19 torr

Solution :

According to the Dalton's law, the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gasses.

P_T=p_{H_2O}+p_{O_2}

where,

P_T = total partial pressure = 805 torr

P_{O_2} = partial pressure of oxygen gas = ?

P_{H_2O} = partial pressure of water = 25.81 mm Hg = 25.81 torr

Now put all the given values is expression, we get the partial pressure of the oxygen gas.

805\text{ torr}=25.81\text{ torr}+p_{O_2}

p_{O_2}=779.19\text{ torr}

Therefore, the partial pressure of oxygen gas is, 799.19 torr

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(a) Calculate the total volume (in liters) of air an adult breathes in a day. (b) In a city with heavy traffic, the air contains
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Answer:

a) V air/day = 8640 L air  an adult breaths / day

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Explanation:

a) one average person has 12 breaths for min:

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in each breath it take an average  of 500 mL on air.

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⇒ 12 breath / min * 500mL air / breath = 6000 mL air / min

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salantis [7]

Answer:

The answer to your question is <u>111 g of CaCl₂</u>

Explanation:

Reaction

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3 years ago
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