CS2 (g) + 4 H2 (g) <====> CH4 (g) + 2 H2S (g)   Calculate the value of Keq if the equilibrium concentrations are [CS2] = 0.140, [H2] = 0.250, [CH4] = 0.0200, and [H2S] = 0.0400.

6 of 12 Part A I Review | Constants Periodic Table Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g) = C(s) + O2(g), Kgoal =? by making use of the following information: 1. 2CO2(g) + 2H2O(1) = CH;COOH(1) + 202(g), K = 5.40 x 10-16 2. 2H2 (g) + O2(g) = 2H,0(1), K2 1.06 x 1010 3. CH3COOH(1) = 2C(s) + 2H2(g) + O2(g), K3 = 2.68 x 10-9 Express your answer numerically. • View Available Hint(s) 中。 goal = 5:08 AM 19 3/1/2021

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

Given these reactions and their equilibrium constants, CO(g) + 3 H₂(g) → CH4(g) + H₂O(g) K = 3.93 N₂(g) + H₂(g) = NH3(g) Kc = 0.324 determine Ke for the following reaction. CO(g) + 2 NH3(g) CH4(g) + H₂O(g) + N₂(g) Your Answer: Kc = 37.4

Given the following reactions and equilibrium constants: (1) HCN(g) + OH* — CN- + H₂O (g) K₁ =4.9 x 104 (2) H₂O(g) H¹(g) + OH- K₂ = 1.0 x 10-14 - What will be the equilibrium constant for: HCN(g) → CN- + H* (g) ? um constant 5.9 x 104 4.9 x 10-10 5.0 x 10-10 4.9 x 10-40 4.9 x 1018

Consider the following equation:                        N2(g) + 2O2(g) + heat  <=>  2 NO2(g)  In what way will the equilibrium shift when the following stresses occur? The temperature is increased.  More N2 is added.  NO2 is collected and removed.  The pressure is increased.