Ask a New Question

Question

If C + CO2 <--> Co, when equilibirum is established at 1000 K, the total pressure in the system is 4.70 atm. If Kp= 1.72, what are the partial pressures of CO and CO2?
14 years ago

Answers

DrBob222
C(g) + CO2(g) ==> CO(g)

Kp = 1.72 = pCO/pCO2
I would set up an ICE chart where p = pressure of CO and 4.70 = pressure CO2 at equilibrium. Substitute into Kp expression and solve for p.
14 years ago

Related Questions

Consider the following equilibrium: PCl5 = PCl3+ Cl2 5.0 moles of are placed in a 10.0... What is the value of the equilibrium constant for the dissociation of acetic acid's proton? What do... The Kp for the following equilibrium system is 4.31 x 10‒4 at 375°C : N2(g) + 3H2(g) ↔ 2NH3(g). If... The value of Keq for the equilibrium H2 (g) + I2 (g) ↔ 2 HI (g) is 794 at 25 °C. What is the v... What is the value of the equilibrium constant at 25°C for the reaction between each of the following... What is the value of the equilibrium constant at 500 °C for the formation of NH 3 according to the... Are the following ratios equilivent? Prove your answer. 3/5=9/11 What is the value of the equilibrium constant for the overall reaction? ​​ AgCl (s) + 2NH3... In the short​ run, the equilibrium price level will---and the nation will experience---gap because d... Why do businesses sek an equilibrium price
Ask a New Question
Archives Contact Us Privacy Policy Terms of Use