A10 liter flask at 298 k contains a gaseous mixture of o2 and co2 at 1 atmosphere. which statement is true for the partial pressures of o2 and co2 if 0.2 mole of o2 is present in the flask? (given the universal gas constant r = 0.082 l∙atm/k∙mol)

The partial pressures of O₂ and CO₂ are 0.489 atm and 0.511 atm respectively.

Explanation:

From the Questions we are given;

Volume = 10 Liter

Temperature = 298 K

Pressure = 1 atm

We need to calculate the partial pressures of O₂ and CO₂

Step 1 : Number of moles of gaseous mixture

Using the ideal gas equation;

PV =nRT, where P is the pressure, V is the volume, n is the number of moles, T is the temperature in K and R is the ideal gas constant (0.082 L∙atm/K∙mol)

Therefore;

Solving for n

Step 2: Moles of CO₂

Total number of moles of the mixture = 0.409 moles

Moles of Oxygen = 0.2 moles

Therefore;

Moles of CO₂ = 0.409 moles - 0.2 moles

                      = 0.209 moles

Step 3: Partial pressures of O₂ and CO₂

Therefore;

Partial pressure of Oxygen gas

Partial pressure of CO₂

Thus, the partial pressures of O₂ and CO₂ are 0.489 atm and 0.511 atm respectively.

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b