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
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
To determine the mass of one liter of C4H10 (butane) at the same temperature and pressure, we need to know the density of butane at that specific condition. Since only the mass of CO2 is provided, we don't have enough information to directly calculate the mass of butane.
The density of a substance can be calculated using the equation:
Density = Mass / Volume
To find the mass of butane, we need to know its density. The density of butane varies depending on the temperature and pressure. Therefore, we would require additional information to determine the density of butane at the given conditions.