Multiple Choice
A gas mixture with a total pressure of 795 mmHg contains CO2 at 107 mmHg, Ar at 255 mmHg, and O2 at 184 mmHg. The mixture also contains helium gas. What mass of helium gas is present in a 12 L container at 298 K?
7. Gases
Partial Pressure
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A mixture of argon and hydrogen gases, in a 6.38 L flask at 90°C, contains 6.37 grams of argon and 0.399 grams of hydrogen. The partial pressure of hydrogen in the flask is ___ atm and the total pressure in the flask is ___ atm. What is the partial pressure of hydrogen in the flask?
A
1.00 atm
B
0.50 atm
C
0.75 atm
D
1.25 atm
Verified step by step guidance1
Convert the given masses of argon and hydrogen to moles using their respective molar masses. The molar mass of argon (Ar) is approximately 39.95 g/mol, and the molar mass of hydrogen (H2) is approximately 2.02 g/mol.
Use the ideal gas law equation, \( PV = nRT \), to find the partial pressure of hydrogen. Here, \( P \) is the pressure, \( V \) is the volume (6.38 L), \( n \) is the number of moles of hydrogen, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin. Convert the temperature from Celsius to Kelvin by adding 273.15 to 90°C.
Calculate the partial pressure of hydrogen by rearranging the ideal gas law to solve for \( P \): \( P = \frac{nRT}{V} \). Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the equation.
Calculate the total pressure in the flask by first finding the partial pressure of argon using the same ideal gas law approach, and then add the partial pressures of argon and hydrogen together.
Compare the calculated partial pressure of hydrogen with the given options to determine the correct answer.
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