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- Calculate ΔG. For the following process at 25°C: BaF2 (s) = Ba2 + (aq) + 2F - (aq) The Ksp of BaF2 is 1.7 x 10^-6 ΔG° = _____ kJ/molWhen 3.0 mole of I2 and 4.0 mole of Br are placed in a 2.0-L rxn chamber at 150 degrees celsius, the following reaction occurs until equilibirum is reached. I2(g) + Br2(g) <--> 2IBr(g) Chemical analysis then shows that the reactor contains 3.2 mole of IBr. What is the equilibrium constant for the reaction ?Suppose that something had gone wrong in the Big Bang, and instead of ord inary hydrogen there was an abundance of deuterium in the universe . There would be many subtle changes in equilibria, particularly the deuteron transfer equilibria of heavy atoms and bases. The Kw for D2O, heavy water, at 25 °C is 1.35 x 10-15. (a) Write the chemical equation for the autoprotolysis (more precisely, autodeuterolysis) of D2O. (b) Evaluate pKw for D2O at 25 ° C. (c) Calculate the molar concentrations of D3O+ and OD- in neutral heavy water at 25 °C . (d) Evaluate the pD and pOD of neutral heavy water at 25 °C. (e) Formulate the relation between pD, pOD, andpKw(D2O).
- Given that E° = +0.897 V, calculate E at 25°C forPb(s) ∣ Pb2+(0.0400 M) ∣∣ Fe3+(0.200 M), Fe2+(0.0100 M) ∣ Pt(s) A) +0.779 VB) +0.935 VC) +1.015 VD) +1.134 V Thank you!What is Ecell at 25°C for the reaction Ca(s) | Ca2+(2.898 M) || Sn2+(0.137 M) | Sn(s)? Report your answer to the hundredths place and do not include units. Half-reaction E° (V) Ca2+ + 2e- → Ca(s) -2.87 Sn2+ + 2e- → Sn(s) -0.14For the reduction 2FeCl3 + SnCl2 =====➔ 2 FeCl2 + SnCl4 in aqueous solution the following data were obtained at 25oC t(min) 1 3 7 11 40 Y 0.01434 0.02664 0.03612 0.04102 0.05058 Where y is the amount of FeCl3 reacted in moles per liter. The initial concentrations of SnCl3 and FeCl3 were respectively, 0.03125, 0.0625 moles/L. a.)Show that the reaction is third order (derive the rate law), and b.) calculate the average specific rate constant.
- The Ksp of PbCl2 is 1.7x10-5 at 25oC. What is DGo? Is it possible to prepare a solution that contains Pb2+(aq) and Cl2(aq), at their standard-state concentrations?A 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
- Zinc may be directly leached from zinc-lead sulphide concentrates by reaction with sulphuricPbS(s) + H2SO4 + 1 O2(g) → PbSO4(solid) + S° + H2O 21ZnS(s) + H2SO4 + 2 O2(g) → ZnSO4(aq) + S° + H2Oacid and oxygen. In addition, lead sulphide will be oxidized to give insoluble lead sulphate:Assume that a plant is to treat 400 t/day of concentrate containing 20.0 weight % Zn as ZnS and 110.0 weight % Pb and PbS. The concentrate and leach solution enters the leaching vessel at 32.0% solids. During the leach, 85.0% of the zinc is extracted and all the lead sulphide is oxidized. After the leaching step, the slurry passes to a thickener.(a) Calculate the concentration of Zn (in g/L) in the solution passing to metal recovery. Assume a solution density of 1.11 g/mL.(b) Calculate the tonnes per day of elemental sulphur produced.NOTE: “% solids†is the solids content of a slurry (consisting of particles and solution) and is defined as…consider the balance to reaction 6 A + 9 B -> 3C + 5D If 6.448 moles of A (MW = 39.34) are consumed, how many moles of B (MW = 42.66) are also consumed?Calculate the emf, E at 298.15 K for the given reaction: Cr2O7 2 – (aq) + 14 H+ (aq) + 6 I – 1 è 2Cr 3+(aq) + 3I2(s) + 7H2O(l) When [Cr2O7 2 – ] = 2.0 M; [H+] = 1.0 M ; [I – 1 ] = 1.0 M ; [Cr 3+] = 1.0x10 – 5 M and [H2O] = 1.0 x 10 – 5 M Calculate the free-energy occurring in the system .