Station 3 Station 4. Station 5. 3BaCl(aq) + 2NaPO(aq)- Baz Poy +_ Nack Balanced Molecular Reaction Equation from above Complete Ionic Reaction Equation Net Ionic Reaction Equation HCl(aq) + NaCO(aq)- Balanced Molecular Reaction Equation from above Complete Ionic Reaction Equation Net Ionic Reaction Equation CuSO SH₂O (s)- Balanced Molecular Reaction Equation from above Complete Ionic Reaction Equation Net Ionic Reaction Equation NaCl()

Station 3 Station 4. Station 5. 3BaCl(aq) + 2NaPO(aq)- Baz Poy +_ Nack Balanced Molecular Reaction Equation from above Complete Ionic Reaction Equation Net Ionic Reaction Equation HCl(aq) + NaCO(aq)- Balanced Molecular Reaction Equation from above Complete Ionic Reaction Equation Net Ionic Reaction Equation CuSO SH₂O (s)- Balanced Molecular Reaction Equation from above Complete Ionic Reaction Equation Net Ionic Reaction Equation NaCl()

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 2ALQ: The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative...

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A student set up an experiment for six different trials of the reaction between 1.00-M aqueous acetic acid, CH3COOH, and solid sodium hydrogen carbonate, NaHCO3. CH3COOH(aq) + NaHCO3(s) NaCH3CO2(aq) + CO2(g) + H2O() The volume of acetic acid was kept constant, but the mass of sodium bicarbonate increased with each trial. The results of the tests are shown in the figure. (a) In which trial(s) is the acetic acid the limiting reactant? (b) In which trial(s) is sodium bicarbonate the limiting reactant? (c) Explain your reasoning in parts (a) and (b).
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations.
Classify each of the reactions according to one of the four reaction types summarized in Table 18.1. (a) C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O() rH = 673 kj/mol-rxn rS = 60.4 j/K mol-rxn (b) MgO(s) + C(graphite) Mg(s) + CO(g) rH = 490.7 kJ/mol-rxn rS = 197.9 J/K mol-rxn TABLE 18.1 Predicting Whether a Reaction Will Be Spontaneous Under Standard Conditions
Explain the meaning of “the reaction goes to less than 100% completion”
fill in the missing reaction component: CuSO4(5H2O) + ______ --> CuSO4 + 5H2O
Which of the following factors can be a reason for yied percentage to be low? 1.Reactant impurities exist 2.The temperature of the reaction vessel is to low 3.The reaction has not been given enough time for completion 4.Two of the above factors can be a reason 5.All three of the above factors can be a reason.
Assume that 1.00 mL (1.02 g) of crude product mixture is obtained from the reactionbefore the washing steps, and the distribution constant of the product mixture in brine isK = (Cmixture/Cbrine) = 50.0. Assuming that after mixing the product mixture volume isstill 1.00 mL (i.e., the volume lost is small), and the volume of the first brine wash layeris 2.00 mL. What mass (grams) of product mixture is lost (dissolves) in the first brinewash? (See Technique 13.2, p 53.) Show work.
Which of the following chemical reactions has a negative ΔS? (The reactions are unbalanced as written - you must balance them!) Group of answer choices Fe(s) + H2O(l) → Fe3O4(s) + H2(g) PCl5(s) + H2O(l) → POCl3(l) + HCl(aq) TiCl4(s) + H2O(g) → TiO2(s) + HCl(g) Ag(s) + H2S(g) + O2(g) → Ag2S(s) + H2O(g)
In the reaction: Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O, S2+ is being reduced. TRUE OR FALSE
Federal regulations set an upper limit of 50 parts per million(ppm) of NH3 in the air in a work environment [that is, 50molecules of NH31g2 for every million molecules in the air].Air from a manufacturing operation was drawn through asolution containing 1.00 * 102 mL of 0.0105 M HCl. TheNH3 reacts with HCl according to: NH3(aq) + HCl(aq)-------->NH4Cl(aq) After drawing air through the acid solution for 10.0 min at arate of 10.0 L/min, the acid was titrated. The remaining acidneeded 13.1 mL of 0.0588 M NaOH to reach the equivalencepoint. (a) How many grams of NH3 were drawn into theacid solution? (b) How many ppm of NH3 were in the air?(Air has a density of 1.20 g/L and an average molar mass of29.0 g/mol under the conditions of the experiment.) (c) Isthis manufacturer in compliance with regulations?
Which of the following chemical reactions has a negative ΔS? (The reactions are unbalanced as written - you must balance them!) Group of answer choices PCl5(s) + H2O(l) → POCl3(l) + HCl(aq) TiCl4(s) + H2O(g) → TiO2(s) + HCl(g) Ag(s) + H2S(g) + O2(g) → Ag2S(s) + H2O(g) Fe(s) + H2O(l) → Fe3O4(s) + H2(g)
The concentration of arsenic in an insecticide can be determined gravimetrically by precipitating it as MgNH4AsO4. The precipitate is ignited and weighed as Mg2As2O7. Determine the %w/w As2O3 in a 1.627-g sample of insecticide that yields 106.5 mg of Mg2As2O7.