A mixture of 0.592 M H₂O, 0.480 M Cl₂O, and 0.747 M HClO are enclosed in a vessel at 25 °C. H₂O(g) + Cl₂O(g) = 2 HOCI(g) Kc = 0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [C!,O]= [HOCI]=

4. For the equilibrium CH₂(g) + 2H₂S(g) = CS₂(g) + 4H₂(g), the concentrations at equilibrium are [CH4] = 0.0804 M, [H₂S] = 0.0608 M, [CS₂] = 0.0196 M, and [H₂] = 0.0784 M at 1400.0 K. Using the equilibrium constant expression from before, calculate Kc.

A mixture of 0.471 M H₂O, 0.431 M Cl₂O, and 0.675 M HClO are enclosed in a vessel at 25 °C. H₂O(g) + Cl₂O(g) = 2 HOCI(g) K = 0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [C!,O]= [HOCI]= MacBook Pro Search or type URL 00 8 A -0 < M M + 11 M del

Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium.  The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M.   CH4(g) + 2H2S(g) ↔  CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.