The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is ________ mm Hg.

Question

Quizplus · Accepted Answer

1. Calculate the number of moles of each gas:  
n(CO2) = 2.34 g / 44.01 g/mol = 0.0531 mol  
n(SO2) = 1.73 g / 64.06 g/mol = 0.0270 mol  
n(Ar) = 3.33 g / 39.95 g/mol = 0.0834 mol

2. Calculate the total number of moles:  
n(total) = n(CO2) + n(SO2) + n(Ar) = 0.1635 mol

3. Use the ideal gas law to calculate the pressure:  
PV = nRT  
P = nRT / V = (0.1635 mol)(0.0821 L·atm/mol·K)(315 K) / 12.2 L = 3.78 atm

4. Convert atm to mm Hg:  
P = 3.78 atm × 760 mm Hg/atm = 2873 mm Hg

5. Round to the nearest whole number:  
P = 263 mm Hg

The Pressure in a 12