For the reaction 2CO2 (g)    ⇌       2CO (g) + O2 (g), Kc = 6.4 x 10-7.  If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g)   1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms   2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown.   3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown.   4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.

Consider the following equilibrium system at 355 K. 2NOBr(g) -----> 2NO(g)+Br2(g). If an equilibrium mixture of the three gases at 355 K contains 3.21x10^-2 M NOBr, 2.01x10^-2 M NO,and 3.98x10^-2 M Br2 what is the value of the equilibrium constant K

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.