Assuming the gas is ideal, we use the ideal gas law:
PV = nRT
where
P = pressure
V = volume
n = number of moles
R = universal gas constant
T = temperature
Note that there are two different species involved, but their P and T are the same (of course, R also). Rewriting the equation isolating the constants,
P/RT = n/V = constant
Therefore, we can equate their n/V ratios since their P/RT are equal. The equation to be used now is
n1 / V1 = n2 / V2
To get the number of moles, we divide the mass by the molar mass. To solve for the molar mass, get a periodic table and add the individual mass of the elements in the chemical formula. The molar mass of CO2 is 1*12 + 2*16 = 44 g/mol, and the molar mass of C4H10 is 4*12 + 10*1 = 58 g/mol.
Substituting,
(1.95 / 44) / 1 = (m / 58) / 1
0.04432 = m / 58
m = 58 * 0.04432
m = 2.57 g C4H10
Hope this helps :3
At a certain Pressure and Temperature one liter of CO2 weigh's 1.95g.
What is the mass of one liter of C4H10 at the same temperature and pressure
1 answer