Consider the following equilibria in aqueous solution: Ag* + Cl <=> ABCI(aq), K-2.0x103 AgCl(aq) + Cl <=> AgCl, K=9.3x101 AgCI(s) <=> Ag* + Cl, K=1.8x10 10 The concentration of AgCl(aq) in equilibrium with undissolved AgCI(s) is:
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- The solubility product constant, Ksp, at 25°C for AgI(s) in water has the value 8.3 × 10–17. Calculate ΔG at 25°C for the process AgI(s) ⟷⟷ Ag+(aq) + I–(aq) where [Ag+] = 9.1 × 10–9 M and [I–] = 9.1 × 10–9 M. (R = 8.314 J/K • mol)A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the equilibrium concentrations for all substances?1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
- A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the value of KC at 800. K?At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3. N2 (g) + O2 (g) NO 2 NO (g) (a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that ofNO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In caseaffirmative or negative, substantiate your answer.(b) If the system is not in equilibrium, in which direction should the reaction proceed?(c) When the system is in equilibrium, what are the equilibrium concentrations?The concentration of calcium carbonate in a sample of water saturated with the solid was found to be 7.00 x 10-5 moldm-3 at 200C. What is the solubility product of calcium carbonate at this temperature?
- The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate unitsA reaction mixture that consisted of 0.20 mol N2(g) and 0.20 mol H2(g) was introduced into a reactor of volume 25.0 L and heated. At equilibrium, 5.0% of the nitrogen gas had reacted. What is the value of the equilibrium constant KC for the reaction N2(g) + 3H2(g) ⇋ 2 NH3(g) at this temperature?Calculate the percentage change in Kx for the reaction H2CO(g) ⇋ CO(g) + H2(g) when the total pressure is increased from 1.0 bar to 2.0 bar at constant temperature.
- Consider two solutions, the first being 50.0 mL of1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH.When the two solutions are mixed in a constant-pressurecalorimeter, a precipitate forms and the temperature of themixture rises from 21.5 to 27.7 °C. (a) Before mixing, howmany grams of Cu are present in the solution of CuSO4?(b) Predict the identity of the precipitate in the reaction.(c) Write complete and net ionic equations for the reactionthat occurs when the two solutions are mixed. (d) From thecalorimetric data, calculate ΔH for the reaction that occurson mixing. Assume that the calorimeter absorbs only a negligiblequantity of heat, that the total volume of the solutionis 100.0 mL, and that the specific heat and density of thesolution after mixing are the same as those of pure water.4.32) Certain bacteria in soil obtain the necessary energy for growth by oxidizing nitrite to nitrate: 2NO2- (aq) + O2 (g) —-> 2NO3- Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, Calculate the amount of Gibbs energy released when 1 mole of NO2- is oxidized to 1 mole of NO3-.The equilibrium constant for the gas-phase isomerization of borneol, C10H17OH, to isoborneol at 503 K is 0.106. A mixture consisting of 6.70 g of borneol and 12 .5 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractionsof the two substances at equilibrium.