Consider the following reaction at 200 °C: 2co(g) + 02(g) = 2C0;(g) An equilibrium mixture contains 0.200 mol CO, 1.30 mol 0z and 0.300 mol CO; in a 500. ml reactor. At a certain instant, a valve is opened, and 0.100 mol of CO, is added to the reactor. I Determine the value of Ke at 200 °C .2 Once equilibrium has been re-established, the concentration of oxygen gas in the reactor was measured to be 2.66 M. Determine the concentration of the other species present in the system for this set of conditions.
Consider the following reaction at 200 °C: 2co(g) + 02(g) = 2C0;(g) An equilibrium mixture contains 0.200 mol CO, 1.30 mol 0z and 0.300 mol CO; in a 500. ml reactor. At a certain instant, a valve is opened, and 0.100 mol of CO, is added to the reactor. I Determine the value of Ke at 200 °C .2 Once equilibrium has been re-established, the concentration of oxygen gas in the reactor was measured to be 2.66 M. Determine the concentration of the other species present in the system for this set of conditions.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Transcribed Image Text:Question 1
Consider the following reaction at 200 °C:
2C0(g) + 02(g) = 2C02(g)
An equilibrium mixture contains 0.200 mol CO, 1.30 mol 0z and 0.300 mol CO; in a 500. mL
reactor. At a certain instant, a valve is opened, and 0.100 mol of COz is added to the reactor.
1.1 Determine the value of Kç at 200 °C
1.2 Once equilibrium has been re-established, the concentration of oxygen gas in the reactor was
measured to be 2.66 M. Determine the concentration of the other species present in the
system for this set of conditions.
Expert Solution
Step 1
The equilibrium reaction taking place is given as,
=> 2 CO (g) + O2 (g) -------> 2 CO2 (g)
Given: Moles of CO at initial equilibrium = 0.200 mol.
Moles of O2 at initial equilibrium = 1.30 mol.
Moles of CO2 at initial equilibrium = 0.300 mol.
Volume of reacted = 500 mL = 0.500 L (Since 1 L = 1000 mL)
And moles of CO2 added = 0.100 mol.
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