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Sagot :
Answer:
a. 21.46atm
b. 0.4737
c.
Mole fraction O2 = 0.1579
Mole fraction CO2 = 0.2105
Mole fraction H2O 0.2105
Mole fraction Ne = 0.4211
Explanation:
a. To solve the total pressure of the cylinder we need to use:
PV = nRT
Where P is pressure: Our incognite
V is volume: 7.80L
n are total moles: 2.700mol + 0.600mol + 2.400mol = 5.700moles
R is gas constant: 0.082atmL/molK
And T is absolute temperature in K: 85°C + 273.15 = 358.15K
P = nRT/V
P = 5.700mol*0.082atmL/molK*358.15K/7.80L
P = 21.46atm
b. Mole fraction of O2 is the ratio of moles of O2 (2.700mol) over total moles of the mixture (5.700mol).
Mole fraction = 2.700mol / 5.700mol = 0.4737
c. In the reaction:
C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)
For a complete reaction of the 0.600mol of C2H4 there are required:
0.600mol C2H4 * (3 mol O2 / 1mol C2H4) = 1.800 moles of O2
As there are 2.700moles of O2, will remain:
2.700 - 1.800 = 0.900moles of O2
All C2H4 is consumed because is limitng reactant and there are produced:
0.600mol C2H4 * (2 mol CO2 / 1mol C2H4) = 1.200 moles of CO2
0.600mol C2H4 * (2 mol H2O / 1mol C2H4) = 1.200 moles of H2O
And 2.400 mol of Ne that doesn't react.
Total moles are:
0.900mol + 1.200mol + 1.200mol + 2.400mol = 5.700mol
Mole fraction O2 = 0.900mol / 5.700mol = 0.1579
Mole fraction CO2 = 1.200mol / 5.700mol = 0.2105
Mole fraction H2O = 1.200mol / 5.700mol = 0.2105
Mole fraction Ne = 2.400mol / 5.700mol = 0.4211
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