A sample of carbon dioxide has a mass of 35.0 g and occupies 2.5 L at 400.0K. What pressure does the gas exert?
2007-05-31 03:23:14 · 3 answers · asked by <3 1 in Science & Mathematics ➔ Chemistry
the equation is PV = nRT
the V = 2.5 L
the T = 400 K
the R is a constant, 0.0821 L atm/mol K
the n is moles, which is mass over molar mass, or
35 g/44 g/mol = 0.795 mol
so P = nRT/V, = (0.795 * 0.0821 * 400) / 2.5 L
the answer is 10.4 atm
2007-05-31 03:28:17 · answer #1 · answered by Verdad 2 · 1⤊ 0⤋
Not a hard question at all. You first convert the mass of CO2 into moles by dividing by the molar mass of CO2.
Then, use the ideal gas law: PV=nRT where P is the pressure, V is the volume, n is the number of moles of CO2, R is the gas constant and T is the temperature in K.
Just plug in your values and solve for P.
2007-05-31 10:26:32 · answer #2 · answered by hcbiochem 7 · 0⤊ 0⤋
PV=NkT, go for it.
2007-05-31 10:26:50 · answer #3 · answered by Del Piero 10 7 · 0⤊ 0⤋