Chemistry - Gas Stoichiometry

Question

How many grams of a gas with a molar mass 36.02 g/mol would be required to occupy a 757 mL flask at 0.960 atm and 92.4 degrees Celcius?

Answer 1

Use the ideal gas law PV = nRT

P = pressure = 0.960 atm

V = volume in L = 757 ml = 0.757 L

n = moles = ?

R = gas constant = 0.0821 Latm/Kmol

T = temp in Kelvin = 92.4C + 273.15 = 365.55

Solve for n (moles)

n = PV / RT = (0.960)(0.757) / (0.0821)(365.55

n = 0.0242 moles

The mass would be 0.0242 moles x 36.02 g /mol = 0.872 g