An Experiment Involving Ideal Gas Law

Calculation of Volume for 3.50 Moles of Chlorine

In chemistry, the ideal gas law is often used to determine various properties of gases. The ideal gas law, PV = nRT, relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas. By manipulating this equation, we can solve for any of these variables if we know the others.

Answer:

To answer the first question, we can use the ideal gas law to find the volume of 3.50 moles of chlorine at 34°C and 2.45 atm. First, we need to convert the temperature to kelvin by adding 273.15 (34°C + 273.15 = 307.15 K). Then we can plug in the values and solve for V:

PV = nRT

V = nRT/P

V = (3.50 mol)(0.08206 L atm mol^-1 K^-1)(307.15 K)/(2.45 atm)

V = 36 L

So 3.50 moles of chlorine at 34°C and 2.45 atm would occupy a volume of 36 L.

Calculation of Molecular Mass for Unknown Gas

For the second question, we can use the ideal gas law to find the number of moles of the unknown gas. Once we know the number of moles, we can use the mass and volume to calculate the molecular mass (molar mass) of the gas.

PV = nRT

n = PV/RT

n = (1.08 atm)(5.75 L)/(0.08206 L atm mol^-1 K^-1)(298.15 K)

n = 0.261 mol

Now we can use the mass and number of moles to calculate the molecular mass:

molecular mass = mass/number of moles

molecular mass = 15.5 g/0.261 mol

molecular mass = 59.4 g/mol

So the molecular mass of the unknown gas is 59.4 g/mol.

The molecular mass of the unknown gas is 59.4 g/mol.