A 10.0-L flask contains 1.031gO2 and 0.572gCO2 at 18°C.
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A 10.0-L flask contains 1.031gO2 and 0.572gCO2 at 18°C. What are the partial pressures of oxygen and carbon dioxide? What is the total pressure? What is the mole fraction of oxygen in the mixture? |
Explanation
First, calculate the number of moles of O2 and CO2.
Since the molar mass of each is not given, calculate using data from Periodic Table.
MMO2 = 32 g/mol
MMCO2 = 44 g/mol
nO2 = 1.031 g/32.0 g/mol
nO2 = 0.0322 mol
nCO2 = 0.572 g/44.0 g/mol
nO2 = 0.0130 mol
Calculate the total number of moles.
ntotal = 0.0322 mol + 0.0130 mol
ntotal = 0.0452 mol
In order to get the total pressure, you may use the ideal gas law.
PV = nRT
Ensure that units are converted correctly.
Ptotal = (ntotal x R x T)/V
Ptotal = [0.0452 mol x (0.08206 L-atm/mol-K) x (18 + 273.15 K)]/10 L
Ptotal = 0.108 atm
You can calculate the mole fraction, X, of O2 using the following formula.
XO2 = nO2/ntotal
XO2 = 0.0322 mol/0.0452 mol
XO2 = 0.712
Answer
Total pressure is 0.108 atm. Mole fraction of oxygen is 0.712.
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