Given:​CS2 (g) + 3 Cl2 (g) < = > CCl4 (g) + S2Cl2 (g)​ DH = – 238 kJ​Using arrows, predict which way the equilibrium will shift (“---->” to products, “

Which is true of a system at equilibrium when Kc < 1? O Equilibrium favors neither reactants or products Equilibrium favors products O Equilibrium favors reactants Equilibrium is shifting to the left Equilibrium is shifting to the right

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?

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Consider the following reaction:COCl2(g) CO(g) + Cl2(g) If 1.64×10-3 moles of COCl2(g), 0.398 moles of CO, and 0.360 moles of Cl2 are at equilibrium in a 18.2 L container at 843 K, the value of the equilibrium constant, Kc, is .

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) A catalyst is added to the reaction mixture. which will happen? the equilibrium will not shift  the equilibrium will shift towards product but keq will not change the equilibrium will shift towards reactant but keq will not change     the equilibrium will shift towards product and keq will increase the equilibrium will shift towards reactant and keq will decrease (b) The total pressure of the system is increased by adding a noble gas.       (c) Cl2(g) is removed from the system.

Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl (aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PbCl2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+: mol/L and Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 10-3 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-³M is kJ/mol. Show your calculations on the separate sheet of paper.

A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) ⥂ 2 SO3 (g) At equilibrium, 0.0916 mol of SO3 is present. a.) What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b.) If the container size is 3.0 L, what is the value of the equilibrium constant?

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease   (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease  (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e)…