Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375X (b) What is Kp if the total pressure is 10.5 atm? 9.12
Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375X (b) What is Kp if the total pressure is 10.5 atm? 9.12
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...
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Transcribed Image Text:Be sure to answer all parts.
A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of
graphite in a closed container until the following equilibrium was reached:
C(s) + CO₂(g) 2 CO(g)
Under these conditions, the average molar mass of the gases was 34.5 g/mol.
(a) Calculate the mole fractions of CO and CO₂.
The mole fraction of CO is
0.40625
The mole fraction of CO₂ is
0.59375 X
(b) What is Kp if the total pressure is 10.5 atm?
9.12
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