CO2 + C (Graphite) ----------> 2 CO
Initially 0.56 0 0
At equili (0.56 - x) x 2x
Keq = [CO]^2/[CO2][C]
2.25 = (2x)^2*/((0.56 - x)(x))
x = 0.2016
At equilibrium,
[CO2] = 0.56 - 0.2016 = 0.3584 M
C(graphite) = 0.2016 M
[CO] = 2x = 2*0.2016 = 0.4032 M
13. Calculate equilibrium concentrations: [CO2] 0.56 CO2(8)+ C(graphite) 2 CO(g) M K=2.25
Consider the following reaction: CO2(g) + C(graphite) ⇌ 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.
1) The following reaction is an equilibrium reaction. CO2(g) + C(graphite) = 2 CO(g) A reactor initially contained only 0.20 atm CO2 gas in the presence of graphite at 25 °C and later the reaction reached an equilibrium. Answer the following questions. A) If Kis 2.25 at the given temperature above, calculate the equilibrium pressures of CO, and CO, respectively. [6 pts) B) Determine the Ke of the reaction above. [4 pts]
13. Given the following reaction: 2CO(g) + O2(g) & CO2(g) with K. = 4000. Ar equilibrium, the concentrations of O, and Co, are 0.10 M and 0.75 M, respectively. Calculate the concentration of CO at equilibrium.
Part A Calculate the equilibrium concentrations of CO2, H2, CO, and H.O at 298 Kif the initial concentrations are CO2-0.700 M and [H] -0.400 M The equilibrium constant for the reaction CO2(x) + H2(g) + CO(x) + H2O(R) is 9.71 x 10 at 298 K Express your answers in moles per liter to three significant figures separated by commas VO AE ? (CO, (H). (CO). [H0] M Denne
Given that K = 3.83 for the reaction C(s,graphite)+ CO2(g) ↔ 2 CO(g) at 606 °C, determine the Gibbs reaction energy (in kJ mol-1) at 606 °C.
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0580 M, [H2] = 0.0430 M, [CO2] = 0.0830 M, and [H2O] = 0.0370 M. (a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.460 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: M CO: M...
Consider the following equilibrium process at 686 ° C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0880 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686 ° C. (b) If we add CO2 to increase its concentration to 0.510 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M...
At 1470 K the value of Kc = 0.0724 for the reaction 2CO(g) ⇋ C (graphite) + CO2(g). CO(g) initially at 2.00 atm is in contact with graphite until equilibrium is reached. What is the partial pressure of CO2(g) at equilibrium?
Based on the following equations: 2 CO2(g) + O2(g) + 2 CO (g) AH- +566.0kJ 2(graphite) + O2(g) + 2 CO (5) AH = -221.0 kJ Determine the enthalpy change (AH) for the following reaction: C(graphite) + O2 (8) CO2(g)
Use Hess's law to determine Ofor the reaction → CO2(g),given that C(graphite) +202(8) — CO(8) A Hº = -110.54 kJ mol C(graphite) + O2(8) —CO2(g) A Hº = -393.51 kJ mol