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All work has to be supplied. You must show the calculations

    All work has to be supplied. You must show the calculations and your answers with full explanationand/or calculation steps. **** All reactions and equilibrium constants are hypothetical. The enthalpies of reaction are alsohypothetical. They are used for your practice and should not be taken as true values. 1: Explain with reason why or why not the following reactions are at equilibrium. A bottle of glue is opened and spread on a piece of paper.2: Explain with reason whether the following reactions would have a high K, a low K, or a K around1.In the ocean, chloride ions join together to make chlorine gas, which is poisonous. 3: The following reactions are at equilibrium. The enthalpy is given. How will the reactions shiftwith the changes listed after. HCO3-(aq) + H+(aq)H2CO3(aq), ΔH = -10kJ/mol. 1) sodium bicarbonate is inserted into thecontainer. 2) carbonic acid is removed. 3) Argon is added to the container. 4) The temperature israised. 5) Sodium hydroxide is added to the container. 4: Look at the following reactions. The initial conditions are stated. Using the reaction quotient,determine which way the reaction will shift. All conditions are given in mol dm-3 unless otherwisestated.Pb+2(aq) + 2OH-(aq)Pb(OH)2(s), Kc= 7×10^19, [Pb2+] = 1.4 x 10^-5, [OH-] = 1.2 x 10^-6, Pb(OH)2 =1gram in one liter.5: Look at the following equilibrium constants for the following reactions. H2(g) + F2(g)2HF(g), Kc = 1.4 x 10^9H2(g) + Cl2(g)2HCl(g), Kc = 1.4 x10^7H2(g) + I2(g)2HI(g), Kc = 1.4x 10^53H2(g) + CO(g)CH4(g) + H2O(l), Kc=1.3×10^-4What is the equilibrium constant for the following reactions? HF(g) + 0.5Cl2(g)HCl(g) + 0.5F2(g)6. Using the initial conditions, determine the equilibrium conditions. All conditions aregiven in mol dm-3 unless otherwise stated. Pb(OH)2(s)Cu+2 (aq) + 2OH—(aq) , Kc= 1.4 x 10-20, [Pb2+] = 5.1 x 10-6, [OH-] = 3.4 x 10-5,Pb(OH)2 = 1gram in one liter. 7.Using the initial conditions, determine the equilibrium conditions. All conditions aregiven in mol dm-3 unless otherwise stated.H2(g) + I2(g)2HI(g), Kc = 1.4 x 105, [H2] = 0.1, [I2] = 0.01, [HI] = 0.5 8. Using the initial conditions, determine the equilibrium conditions. All conditions aregiven in mol dm-3 unless otherwise stated.CO2(g) + CaO(s)  CaCO3(s), Kc = 1.2 x 10-8, [CO2] = 3 x 10-4. Inside the one liter container,there is 40 grams of calcium oxide and 10 grams of calcium carbonate. 9. Change the following Gibbs Energies into Kc. Assume the temperature is at room temperature.A) 112kJ/molB) 12 kJ/molC) -10kJ/molD) 54 kJ/mol 10: Find the rate constant of the reverse reaction for the following. Kc = 8 x 102. The rate constant of the forward reaction is 10.

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