Chem 1465 1st EditionExam # 4 Study Guide 1. For the following endothermic reaction: CaO(s) + CO2 (g) → CaCO3 (s) write shift left, shift right, or no effect to indicate what will happen when:A. More CO2 is added to the system __________B. More CaCO3 is added to the system __________C. The temperature is increased ____________D. The pressure is increased _____________2. Write the expression for K (equilibrium constant) for each of the reactions.A. CO(g) + ½ O2 (g) → CO2 (g)B. 4Fe(s) + 3O2 (g) → 2Fe2O3 (s)3. Determine the temperature range for which each of the following systems would be spontaneousA. ΔH = 350 KJ and ΔS = 150 J/K B. ΔH = 210 KJ and ΔS = -250 J/K 4. Predict whether ΔS is positive, negative, or approximately equal to zero for each processA. A liquid evaporating __________B. Two liquids react to form a gas and a solid __________C. Two gases react to form a gas and a liquid ____________D. A gas and a liquid forming a solid and a gas __________5. For the following pairs in a galvanic cell indicate which is the cathode.A. Fe/Fe2+ and SHE ___________B. Ag/Ag+ and SHE __________6. Balance the following redox reactionsA. IO2+ + NO2+ → NO + I7+ B. V +SO2+ → SO +V3+7. A reaction has a value of Eᵒcell = 0.93 V when Ag│Ag+ is used as a cathode at 298K.A. Find the standard reduction potential of the anodeB. Write the standard galvanic cell notation8. When the concentration of Cr3+ is 0.100 M and of Q2+ is 0.0047 M, the voltage measured under those conditions for Cr│Cr3+││ Q2+│Q galvanic cell is 0.41 V. A. Calculate the value of EcellB. What element is Q?9. Calculate the value of the equilibrium constant (K) for H2PO4 +H2 → PO2 + 2H2O given:H2O + PO3 → H2PO4 K= 7.0 x 106O2 + 2H2 → 2H2O K= 2.0 x 1025PO2 + ½ O2 → PO3 K= 1.0 x 10-910. The following reaction is used commercially to produce hydro bromic acid: H2(g) + Br2(g) → 2HBr (g) K= .150. A chemist takes a sample of HBr and puts it in an empty flask and measures the pressure of it to be 0.500 atm. Determine the pressure of each gas at equilibrium. 11. Calculate the pH of a 0.044 M HClO4 solution.12. A sample of 0.25 M of a weak acid is found to have an equilibrium pH of 3.55. Calculate the K of this
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