Create the Ksp expression for the dissolution of AgCl by dragging the elements and their charges, plus any exponents, to their appropriate positions.

What are the concentrations of PCL5,PCL3, and Cl2 in an equilibrium mixture produced by the decomposition of a sample of pure PCL5 with [PCL5] = 2.00M PCL5(g) = PCL3(g) + Cl2(g) Kc = 0.0211

For the system: 2 HI(g) = H2(g) + 12(g), at 445°C, the value for K, is 0.020. A mixture of H2, 12, and HI in a vessel at 445°C has the following concentrations: [HI] = 2.0 mol/L, [H2] = 0.50 mol/L and [I2] = 0.10 mol/L %3D %3D %3D Which one of the following statements about Q. is TRUE for the above system? Qc = Kc; the system is at equilibrium %3D O Qc is less than Ke; so more H2 & 12 will form OQc is less than Ke; more HI will form Qc is greater than Kc; more H2 and I2 will form

Consider the reaction network of the gaseous isomerisation, decomposition anddimerisation reactions of the same reactant A:Isomerisation: A ⇆ IDecomposition: A ⇆ B + CDimerisation: 2A ⇆ DAt the reaction temperature, the equilibrium constants, expressed in terms of partial pressures, are:Isomerisation: KI = 5Decomposition: KDe = 0.5 barDimerisation: KDi = 5 bar-1At 1 bar, there is only 1 mol of A initially. Express the mole-fraction of each reaction component at equilibrium as function of the extents of the three reactions at equilibrium, ξI, ξDe, ξDi.Calculations resulted in the following values of the extents of the three reactions, isomerisation, decomposition and dimerization at equilibrium: ξI= 0.5400 mol, ξDe =0.2553 mol, ξDi= 0.0483 mol.Calculate the equilibrium mole-fractions of reaction components A, I, B, C and D and show that the equilibrium extent values are correct.

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PC1,(g) + Cl, (g) → PCI, (g) An equilibrium mixture at 450 K contains P(PCI3) = 0.202 atm and P(Cl2) = 0.256 atm and P(PCI5) = 3.45 %3D %3D What is the value of Kp at this temperature? O 2.99 O 7.54 O 66.7 O 1.50 x 102 O 1.78 x 10

The equilibrium constant for the reaction H2+122HI Is 20 at 40 °C, and the vapor pressure of solid iodine is 0.1 bar at that temp. If 12.7 g of solid iodine are placed in a 10-dm³ vessel at 40 °C, what is the minimum amount of hydrogen gas that must be introduced in order to remove all the solid iodine?

find Po2

Will the stress cause the equilibrium to shift towards reactants or products, or will it have no effect? PCI5(9) = PC|3(9) + Cl2c9) ΔΗ > 0 Stress: Increase Volume A. Reactants B. Products C. No Change

Ethyl acetate, acetate and ethanol were added to water solution in concentrations of 0.3M and left at 25°C until the solution reached an equilibrium state: ethyl acetate = 0.276 M;acetate = 0.012 M;ethanol = 0.012 M; The experiment was repeated at the same temperature with the initial concentration of 0.6M of ethyl acetate. a) What will the concentration of acetate be (in moles/liter) once equilibrium is achieved? b) What will the concentration of Ethyl acetate be (in moles/liter) once equilibrium is achieved?

Gas Initial Concentration (M) H2 0.030 I2 0.015 HI ? Samples of three gases, H2(g) , I2(g) , and HI(g) , were combined in a rigid vessel. The initial concentrations of H2(g) and I2(g) are given in the table above. (a) The original value of the reaction quotient, Qc , for the reaction of H2(g) and I2(g) to form HI(g) (before any reactions take place and before equilibrium is established), was 5.56 . On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas.   Equilibrium was established at a certain temperature according to the following chemical equation. H2(g)+I2(g)⇄2HI(g)ΔH°rxn=−9.4kJ/molrxn;Kc=49 After equilibrium was established, the concentration of H2(g) was 0.020M . (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part ( a ). The curves must show how the concentration of each of the three gases changed…