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denpristay [2]
3 years ago
13

Show the calculation of the mass (grams) of a 14.5 liter gas sample with a molecular weight of 82 when collected at 29°C and 740

mm
Chemistry
1 answer:
mote1985 [20]3 years ago
4 0

Answer:

In this conditions, the gaswll weight 46.74 g.

Explanation:

The idal gas law states that:

PV = nRT,

P: pressure = 740 mmHg = 0.97 atm

V: volume = 14.5 L

n: number of moles

R: gas constant =0.08205 L.atm/mol.K

T: temperature = 29°C = 302.15K

n = \frac{PV}{RT} \\n = \frac{0.97x14.5}{0.082 x 302.15 } \\n = 0.57 mol

1 mol gas ___ 82 g

0.57 mol gas __ x

x = 46.74 g

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Answer:

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Explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

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K_H = Henry's constant = 1.40\times 10^{-3}mol/L.atm

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Putting values in above equation, we get:

C_{Ar}=1.40\times 10^{-3}mol/L.atm\times 0.430 atm\\\\C_{Ar}=6.02\times 10^{-4}mol/L

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3 years ago
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