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The answer for the following problem is mentioned below.
- <u><em>Therefore the final volume of the gas is 52.7 ml.</em></u>
Explanation:
Given:
Initial pressure (
) = 290 kPa
Final pressure (
) = 104 kPa
Initial volume (
) = 18.9 ml
To find:
Final volume (
)
We know;
From the ideal gas equation;
P × V = n × R × T
where;
P represents the pressure of the gas
V represents the volume of gas
n represents the no of the moles
R represents the universal gas constant
T represents the temperature of the gas
So;
P × V = constant
P ∝ 
From the above equation;

represents the initial pressure of the gas
represents the final pressure of the gas
represents the initial volume of the gas
represents the final volume of the gas
Substituting the values of the above equation;
= 
= 52.7 ml
<u><em>Therefore the final volume of the gas is 52.7 ml.</em></u>
a) The total pressure of the system is 1.79 atm
b) The mole fraction and partial pressure of hydrogen is 0.89 and 1.59 atm respectively
c) The mole fraction and the partial pressure of argon is 0.11 and 0.19 atm.
<h3>What is the total pressure?</h3>
We know tat we can be able to obtain the total pressure in the system by the use of the ideal gas equation. We would have from the equation;
PV = nRT
P = pressure
V = volume
n = Number of moles
R = gas constant
T = temperature
Number of moles of hydrogen = 14.2 g/2g = 7.1 moles
Number of moles of Argon = 36.7 g/40 g/mol
= 0.92 moles
Total number of moles = 7.1 moles + 0.92 moles = 8.02 moles
Then;
P = nRT/V
P = 8.02 * 0.082 * 273/100
P = 1.79 atm
Mole fraction of hydrogen = 7.1/8.02 = 0.89
Partial pressure of hydrogen = 0.89 * 1.79 atm
= 1.59 atm
Mole fraction of argon = 0.92 / 8.02
= 0.11
Partial pressure of argon = 0.11 * 1.79 atm
= 0.19 atm
Learn more about partial pressure:brainly.com/question/13199169
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