Chemistry help?

Question

Oxygen and Sulfur dioxide react at high pressure and temperature to produce sulfur trioxide as shown in the following chemical equation : SO2(g) + O2 yield SO3
a) Write the balanced equation for this equation
b) The formula weight of the molecule of O2 is ________uma
c) How many moles of O2 do you have in 69.4g of this gas?
d) Assume a sample of 69.4g of O2 gas is contained in a 13.6L vessel at 200degrees. What is the pressure of the O2 in the vessel?
e) Assume that you want to convert all the oxygen in the vessel mentioned above into SO3, how many moles of SO2 would react with all the oxygen in the vessel.
f) Calculate the molar fraction of each gas in the mixture. total number of moles, molar fraction of O2, Molar fraction of SO2.
g) What is the total pressure of the gas mixture in the vessel?
h) How many moles of SO3 would be produced assuming 100% yield for the reaction of O2 and SO2.
g) What is the final pressure SO3 in the vesselassuming100% yield for the reaction.

Answer 1

a)2 SO2 + O2 >> 2SO3

b)31.9988 uma = 32 uma
c)69.4 /32 = 2.17 moles

d) 200°C = 473 K
p(O2) = nRT / V = 2.17(0.08206) 473 /13.6= 6.19 atm

e) the ratio between SO2 and O2 is 2 : 1 so we need
2(2.17)=4.34 moles and we willi have 4.43 moles SO3

f) total moles = 2.17 + 4.43+4.43=11.03
molar fraction O2 = 2.17 / 11.03 = 0.197
molar fraction SO2 = molar fraction SO3 = 4.43 / 11.03 = =0.402

g) p = nRT / V =11.03(0.08206)473 /13.6 = 31.48 atm

h) 4.43

g) p = 4.43 (0.08206)473 / 13.6 =12.6