Asked by Captain
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
What is the mass of one liter of C4H10 at the same temperature and pressure
Answers
Answered by
Jai
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
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