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drek231 [11]
3 years ago
10

When a chemist collects hydrogen gas over water, she ends up with a mixture of hydrogen and water vapor in her collecting bottle

. If the pressure in the collecting bottle is 97.1 kilopascals and the vapor pressure of the water is 3.2 kilopascals, what is the partial pressure of the hydrogen?
Chemistry
1 answer:
gizmo_the_mogwai [7]3 years ago
4 0

Answer: The partial pressure of the hydrogen gas is 93.9 kiloPascals.

Explanation:

The partial pressure of the water vapors = p_{H_2O,g}=3.2 kPa

The partial pressure of the hydrogen gas = p_{H_2}

The pressure measured in the collecting bottle  = p=97.1 kPa

While collecting the hydrogen gas in a collecting bottle with amount of water vapors also get introduced. The total pressure in the collecting bottle will be due to partial pressures of the water vapors and hydrogen.

p=p_{H_2O,g}+p_{H_2}

97.1 kPa=3.2 kPa+p_{H_2}

p_{H_2}=97.1 kPa-3.2 kPa=93.9 kPa

The partial pressure of the hydrogen gas is 93.9 kiloPascals.

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Using the van der waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 c is____________at
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Answer:

D. 1.48atm

Explanation:

Van der waals equation is given as:

(P +an²/v²) (v - nb) = nRT

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R = gas constant (0.0821 Latm/molK)

a and b = gas constant specific to each gas

T = temperature (K)

n = number of moles

According to the given information; V = 22.4L, T = 0.00°C (273.15K), R = 0.0821 Latm/molK, a = 6.49L^2-atm/mol^2, b = 0.0562 L/mol, n = 1.5mol

Hence;

(P + 6.49 × 1.5²/22.4²) (22.4 - 1.5×0.0562) = 1.5 × 0.0821 × 273.15

(P + 6.49 × 2.25/501.76) (22.4 - 0.0843) = 33.638

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