CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO2 in the container was ________ atm.
To calculate the partial pressure of CO2 in the container, we first need to determine the moles of each gas present using the ideal gas law equation:
PV = nRT
First, let's calculate the moles of CO and CO2:
For CO:
nCO = m/MW
where:
m = mass of CO = 5.00 g
MW = molar mass of CO = 28.01 g/mol
nCO = 5.00 g / 28.01 g/mol = 0.1785 mol
For CO2:
nCO2 = m/MW
where:
m = mass of CO2 = 5.00 g
MW = molar mass of CO2 = 44.01 g/mol
nCO2 = 5.00 g / 44.01 g/mol = 0.1136 mol
Now, let's calculate the total moles of gas in the container:
ntotal = nCO + nCO2
ntotal = 0.1785 mol + 0.1136 mol = 0.2921 mol
Next, let's use the ideal gas law to calculate the partial pressure of CO2:
PV = nRT
P = nRT/V
P = (nCO2)RT/V
Now, we need to convert the temperature to Kelvin:
T = 50.0 °C + 273.15 = 323.15 K
Plugging in the values:
P = (0.1136 mol)(0.0821 L.atm/mol.K)(323.15 K) / 0.750 L
P ≈ 3.10 atm
Therefore, the partial pressure of CO2 in the container is approximately 3.10 atm.