For a mixture of CO and CO2, d = 1.50 g/litre 

P = 730 / 760 atm, T = 303K 

PV =w / m RT; PV w / Vm RT 

730 / 760 = 1.5 / m × 0.0821 × 303 =∴ 38.85 

i.e. molecular weight of mixture of CO and CO2= 38.85 

Let % of mole of CO be a in mixture then 

Average molecular weight = a × 28 + (100 – a) 44 / 100 

38.85 = 28a + 4400 – 44a / 100 

a = 32.19 

Mole % of CO = 32.19 

Mole % of CO2= 67.81

To determine the composition of the mixture of CO and CO2, we need to use the ideal gas law and the concept of partial pressures.



First, let's convert the given temperature from Celsius to Kelvin:

T = 30°C + 273.15 = 303.15 K

Next, let's convert the given pressure from torr to atmospheres (atm):

P = 730 torr / 760 torr/atm = 0.9618 atm



The total pressure of the mixture is the sum of the partial pressures of CO and CO2:

Ptotal = PCO + PCO2

We can express the partial pressure of each gas in terms of its mole fraction and the total pressure:

PCO = (XCO)(Ptotal)
PCO2 = (XCO2)(Ptotal)



The mole fraction of a gas is the ratio of the number of moles of that gas to the total number of moles in the mixture. Since density is given, we can use it to calculate the number of moles of the mixture.

The density of the mixture is given as 1.5 g/L. Since the molar mass of CO is 28 g/mol and that of CO2 is 44 g/mol, we can calculate the number of moles using the equation:

1.5 g/L = (nCO * 28 g/mol + nCO2 * 44 g/mol) / 1 L

Simplifying, we get:

nCO * 28 g/mol + nCO2 * 44 g/mol = 1.5 mol



We now have two equations and two unknowns: PCO, PCO2, nCO, and nCO2. We can solve these equations simultaneously to find the values.

Using the ideal gas law, PV = nRT, we can rewrite the equations as:

PCO = (XCO)(Ptotal) = (nCO * RT) / V
PCO2 = (XCO2)(Ptotal) = (nCO2 * RT) / V

Substituting the values and rearranging, we get:

PCO = (nCO * 0.0821 atm·L/mol·K * 303.15 K) / 1 L
PCO2 = (nCO2 * 0.0821 atm·L/mol·K * 303.15 K) / 1 L

Now, we have four equations with four unknowns:

Ptotal = PCO + PCO2
nCO * 28 g/mol + nCO2 * 44 g/mol = 1.5 mol
PCO = (nCO * 0.0821 atm·L/mol·K * 303.15 K) / 1 L
PCO2 = (nCO2 * 0.0821 atm·L/mol·K * 303.15 K) / 1 L

We can