CO(g) + 3H2(8) CHale) + H20(e) What is the concentration of all species at equilibrium if...
ice box quadraric formula please show work and write neat to understand. What is the concentration of all species at equilibrium if the initial concentrations were 0.10 M for CO2 and 0.30 M for HZ? K=25. CO(g) + H2O(g) CO2(g) + H2(g) Initial Change Equilibrium
5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the gases at equilibrium for the reaction: CO(g) + H20 (g) = CO2(g) + H2 (g) Given that the initial concentrations of all the gases are 0.05 M and that Kc = 5.1 at 700 K.
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...
For the following reaction, calculate the equilibrium concentration of CO (g). CO2 (g) + H2 (g) CO (g) + H20 (g) Kc = 0.11 [CO2] = 0.25 M [H2] = 0.80 M [H2O) = 0.50 M
For the reaction N2(g)+3H2(g)⇌2NH3(g) what is the value of Kc at 500 ∘C if the equilibrium concentrations are as follows: [H2] = 0.45 M , [N2] = 0.50 M , and [NH3] = 2.0 M ?
please show all steps. The decomposition reaction of COC12 is, COCldg,-CO(g) + Cl2(g) Kc = 2.2 × 10-10. The initial concentration of CoCl is 0.3166 M 3. the (a) At equilibrium, the concentrations of the products are concentration of reactant. (A) greater than (B) less than (D) unknown because more information is needed to determine. (C) equal to (b) Fill the ICE table below COC: Ico Initial concentration (M) Changes (M) Equilibrium concentration (M) -x (c) Calculate the equilibrium concentration...
For the reaction N2(g)+3H2(g)⇌2NH3(g) what is the value of Kc at 500 ∘C if the equilibrium concentrations are as follows: [H2] = 0.35 M , [N2] = 0.40 M , and [NH3] = 1.8 M ?how to solve answer?
Consider the following reaction: N2(g)+3H2(g)⇌2NH3(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (K) [N2] [H2] [NH3] [Kc] 500 0.115 0.105 0.439 − 575 0.105 M − 0.128 M 9.6 775 0.130 M 0.145 M − 0.0584 Find Kc at 500 K. Find [H2] at 575 K. Find [NH3] at 775 K.
Calculate KC in terms of molar concentration for the reaction N2(g) + 3H2(g) 2NH3(g) when the equilibrium concentration moles per liter are: N2 = 0.02, H2 = 0.01, NH3 = 0.10.