Calculate the value of Kp for the equation C(s) + CO2(g) <--> 2CO(g) Kp = ? Given that at a certain temperature C(s) + 2H2O(g) <--> CO2(g) + 2H2(g) Kp1 = 3.97 H2(g) + CO2(g) <--> H20(g) + CO(g) Kp2 = 0.623
The reaction CO2(g) + C(s) <-> 2CO(g) has a Kp=5.78 at 1200k Delta n for the reaction is ___ Kc for the reaction is ____ 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. Is the reaction at equilibrium? Will more of the solid form, or will some of the existing solid decompose? 3) Consider the following reaction: CH3OH (g) <-> CO (g)...
Calculate the value of Kp for the equation C(s)+CO2(g)−⇀↽−2CO(g)Kp=? given that at a certain temperature C(s)+2H2O(g) −⇀↽−CO2(g)+2H2(g)Kp1=3.73H2(g)+CO2(g) −⇀↽−H2O(g)+CO(g)Kp2=0.689
1. calculate Kp for the reaction C(s) + Co2(g) = 2Co(g at 1300 k and 1 atm, the equilibrium mixture contains 85% co and 10.5% co2 by volume. 2. calculate the partial pressure of Co2 if Pco is changed to 10^-3 ATM.
The reaction CO2(g) + C(s)<-->2CO(g) has Kp=5.78 at 1200 K. 1) Calculate the total pressure at equilibrium when 4.73g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 3.75g of graphite. (I have the answer to this half 1.77 atm) 2) Repeat the calculation of part A in the presence of 0.49g of graphite.
3. At 850°C, Kp is 14.1 for the reaction C(graphite) + CO2(g) t 2CO(g) A reaction vessel at 850°C initially contains CO2 at 0.500 atm, CO at 1.00 atm, and graphite. Determine a. The direction in which the reaction moves b. The equilibrium partial pressure of each gas
Question 1 In the reaction: CO2(g) + C(s) --> 2CO(g), how might the concentration of C(s) (graphite) affect the equilibrium concentration of the product CO(g)? a. It does not affect it at all because C(s) is not included in the expression of the equilibrium constant. Thus, whether C(s) is present or not does not affect the reaction. b. It doesn't affect it as long as there is C(s) present during the reaction (i.e. C(s) is in excess so it does...
Consider the reaction C(s)+CO2(g)⇌2CO(g). When 1.66 mol of CO2 and an excess of solid carbon are heated in a 21.2 L container at 1100K, the equilibrium concentration of CO is 7.19×10−2 M . Part A What is the equilibrium concentration of CO2? Part B What is the value of the equilibrium constant Kc at 1100 K?
Consider the heterogeneous equilibrium process: C(s) + CO2(g) ⇆ 2CO(g) At 700°C, the total pressure of the system is found to be 1.50 atm. If the equilibrium constant (KP) is 1.52, calculate the equilibrium partial pressures of CO and CO2.
For which reaction will Kp = Kc? C(s) + O2(g) ⇌ CO2(g) 2 H2O(l) ⇌ 2 H2(g) + O2(g) CaCO3(s) ⇌ CaO(s) + CO2(g) H2CO3(s) ⇌ H2O(l) + CO2(g) 2 HgO(s) ⇌ Hg(l) + O2(g)