1.)A gas mixture contains 74% nitrogen and 26% oxygen.If the total pressure is 1
ID: 1007876 • Letter: 1
Question
1.)A gas mixture contains 74% nitrogen and 26% oxygen.If the total pressure is 1.02 atm what are the partial pressures of each component? Express your answers using two significant figures. Enter your answers numerically separated by a comma.
2.) The mass of an evacuated 265 mL flask is 143.147 g . The mass of the flask filled with 267 torr of an unknown gas at 35 C is 144.197 g . Calculate the molar mass of the unknown gas.
3..)Consider the following reaction: 2SO2(g)+O2(g)2SO3(g)
a. What is the theoretical yield of SO3?
b.If 131.8 mL of SO3 is collected (measured at STP), what is the percent yield for the reaction?
Explanation / Answer
PT = PN2 +PO2
1.02 = PN2 +PO2
PN2 = 0.74*1.02 = 0.75atm
PO2 = 0.26*1.02 = 0.2652atm
2. PV = nRT
n = W/M
P = 267torr = 267/760 = 0.35atm
V = 265ml = 0.265L
W = 144.197g
T =35C0 = 35+273 =308K
R = 0.0821L-atm/mole-K
PV = WRT/M
M = WRT/PV
= 144.197*0.0821*308/0.35*0.265 = 39312g/mole
3. 2SO2(g)+O2(g)2SO3(g) but missing the data
volume of SO3 is at STP = 2*22400ml = 44800ml
percentage yield = Actual yield*100/Theoretical yield
= 131.8*100/44800 = 0.29%
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