6. The equilibrium constant (Kp) for the reaction C(s) + CO₂(g) →2CO(g) is 1.9 at 727°C. What total pressure must be applied to the reacting system to obtain 0.012 mole of CO2 and 0.025 mole of CO? 7. For the reaction 2CH4(g) C₂H2(g) + 3H₂(g) Kc = 0.150 at 1528 °C. What is the Kp at this temperature?

6. The equilibrium constant (Kp) for the reaction C(s) + CO₂(g) →2CO(g) is 1.9 at 727°C. What total pressure must be applied to the reacting system to obtain 0.012 mole of CO2 and 0.025 mole of CO? 7. For the reaction 2CH4(g) C₂H2(g) + 3H₂(g) Kc = 0.150 at 1528 °C. What is the Kp at this temperature?

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

Chapter1: Chemical Foundations

Section: Chapter Questions

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6. The equilibrium constant (Kp) for the reaction
C(s) + CO₂(g) → 2CO(g)
is 1.9 at 727°C. What total pressure must be applied to the reacting system to obtain 0.012 mole of CO₂
and 0.025 mole of CO?
7. For the reaction 2CH4(g) C₂H2(g) + 3H₂(g)
Kc =0.150 at 1528 °C. What is the Kp at this temperature?

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