The equilibrium constant at 25 °C for the dissolution of silver iodide is 8.5 × 10–17. AgI (s) D Ag+ (aq) + I– (aq) If an excess quantity of AgI(s) is added to water and allowed to equilibrate, what is the equilibrium concentration of I–?

Kc=?

Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 K = (CH3)3N(aq) + H₂O(1) — (CH3)3 NH+ (aq) + OH¯(aq)

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.

What is the equilibrium constant expression for the reaction:3 Fe(s) + 4 H2O (g)⟷  Fe3O4 (s) + 4 H2 (g)

Write the equilibrium constant expression for this reaction: 2CH,COO (aq)+C,H,O,(aq) → C,H1,0,(aq)+2OH¯(aq)

Predict the effect of adding H2O liquid to the equilibrium reaction 

You are on a new planet and discover a substance, Z2O that undergoes autoionization just like water on Earth.  Z2O + Z2O  ⇌ Z3O+ + OZ– Through a series of experiments, you determine the equilibrium constant (Kx) for this autoionization reaction at various temperatures. The value of Keq at 25.1ºC is 6.6 x 10-13. What is the pZ of the pure substance at this temperature? (pZ = -log(Z3O+) Report your answer to the hundreths place.

At a certain temperature, the equilibrium constant for the chemical reaction shown is 6.46 × 10¬³. At equilibrium, the concentration of AB is 3.125 M, the concentration of BC is 1.425 M, and the concentration of AC is 0.210 M. Calculate the concentration of B at equilibrium. AB(aq) + BC(aq) = AC(aq) + 2 B(aq) [B] = M

An equilibrium constant of special importance in much aqueous chemistry is that of the autoionization of water: 2 H₂O (/) H3O+ (aq) + OH¯ (aq) Kw The value of this equilibrium constant at three temperatures near standard temperature is Kw(293 K) = 0.67 × 10-¹4 M² Kw(298 K) = 1.00 × 10-¹4 M² Kw(303 K) = 1.45 × 10-¹4 M² (a) Assuming that the value of AH° and AS° are constant over this narrow temperature range, determine their values (in kJ/mol and J/mol-K, respectively for the ionization equilibrium at 298 K based on this information. (Hint: You should use both the relationship between AG° and K, and the relationship between the Gibbs energy, enthalpy, and entropy in this problem. Setting up your analysis as a least-squares linear fit provides the best result.) (b) Based on the results from part (a), what would you expect the autoionization equilibrium constant to be near the freezing point of water, at T = 275 K?