Total pressure of the system at equilibrium is 4.8 atm at 700 °C and K = 0.019 mol L for the given reaction. Calculate the partial pressure of CO(g) at equilibrium. C(s) + CO,(g) = 2 CO(g) O a. 1.30 atm O b. 1.73 atm Oc. 2.05 atm O d. 1.49 atm O e. 1.96 atm

Total pressure of the system at equilibrium is 4.8 atm at 700 °C and K = 0.019 mol L for the given reaction. Calculate the partial pressure of CO(g) at equilibrium. C(s) + CO,(g) = 2 CO(g) O a. 1.30 atm O b. 1.73 atm Oc. 2.05 atm O d. 1.49 atm O e. 1.96 atm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 129MP: A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A...

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Question

Total pressure of the system at equilibrium is 4.8 atm at 700 °C and K. = 0.019 mol L" for the given reaction. Calculate the partial pressure of CO(g) at equilibrium.
C(s) + CO2(g) = 2 CO(g)
O a. 1.30 atm
O b. 1.73 atm
O . 2.05 atm
O d. 1.49 atm
O e. 1.96 atm

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