Calculate the masses of (i) KNO3 and, separately, (ii) Ba(NO3)2 to add to a 0.110 mol kg−1 solution of KNO (aq) containing 500 g of solvent to raise its ionic strength to 1.00.

Ag(+aq) + Cl-(aq) AgCl(s) ∆H = +112 kJIf ions are colorless, and AgCl is whiteWill the reaction appear “colorless” or “white” if:a) Some of the AgCl (s) is removed?b) The pressure is decreased?c) The temperature is raised?

4. The standard electromotive force of the cell Pt(s) H2(g)|HCl(aq)|AgCl(s)|Ag(s) has been determined from 0°C to 90°C, and the data were found to fit the expression E*/V = 0.237-4.856 × 10-4T(°C) - 3.421 × 10-T²(°C) + 5.869 × 10-ºT³ (°C) Calculate the equilibrium constant, the standard reaction Gibbs energy, entropy and enthalpy for the cell reaction at 25°C. F = 96485 C mol-¹ AgCl(s) + H2(g) → Ag(s) + HCl(aq)

The decomposition of a generic diatomic element in its standard state is represented by the equation X₂(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.71 kJ - mol-¹ at 2000. K and −55.51 kJ · mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG₁ = 4.71 kJ · mol-¹. What is K at that temperature? K at 2000. K= At 3000. K, AGf = −55.51 kJ - mol-¹. What is K at that temperature? K at 3000. K =