Calculate the standard potential of the cell whose overall cell reaction is Zn(s) +2Fe+ (ag) Zn (aq) - 2Fe?+ (aq) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Standard Potential, E (V) Zn+ (ag) + 2e = Zn(s) -0.763 Fet (aq) +e - Fet (aq) 0.771 Standard potential V

Calculate the standard potential of the cell whose overall cell reaction is Zn(s) +2Fe+ (ag) Zn (aq) - 2Fe?+ (aq) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Standard Potential, E (V) Zn+ (ag) + 2e = Zn(s) -0.763 Fet (aq) +e - Fet (aq) 0.771 Standard potential V

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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11. From the balanced molecular equations, write the complete ionic and net ionic equations for the following: (a) K2 C2 04(aq) + Ba(OH)2(aq) – 2KOH(aq) + BaC2 04(s) (b) Pb(NO3)2(aq) + H2 SO4(aq) – PbS04(s) + 2HNO3(aq) - (c) CaCo3(s) + H2 SO4(aq) – CaS04(s) + CO2(g) + H2 O(1)
A 19.51 g sample of impure methylamine, which contains 72.58% (by mass) of CH;NH: , is reacted with 30.81 g of pure oxygen gas: 2.1 4CH, NH,(2) + 90,(8) - 4C0,(8) + 10H,0(?) + 2N;(8) 2.1.1 What is the percentage yield of this reaction if 5.54 g of nitrogen gas is collected? 2.1.2 In another experiment, this impure methylamine was used as follows: • An unknown mass of the impure compound is dissolved in enough water to make 500.0 m of solution. • 20 ml of this solution was transferred by pipette to a clean 250 ml volumetric flask and made up to the mark. • The molarity of the CH;NH; in the final solution was determined to be 0.103 M. Determine the mass of CH;NH; present in the original amount of impure compound used make this solution.
In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the following: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l) (a) Balance the equation. (b) Calculate the theoretical yield of NaF. (c) If 0.792 g of NaF is formed, calculate the percent yield.
2. In the laboratory, O2(g) can be obtained from the following thermal decomposition reaction of potassium chlorate (KCIO3) with the aid of catalyst: A, MnO2 (catalyst) 2KC1O;(s) > 2KCI(s) + 302(g) To determine the composition of the mixture of KCIO3 and potassium chloride (KCI), 0.612 g KCIO3/KCl mixture is taken into a test tube and heated in the presence of sufficient catalyst, MnO2. The total mass of the test tube after heating decreased by 0.096 g. According to this result, what is the percentage of the KCIO3 in the mixture? (K: 39.0 g/mol, Cl: 35.5 g/mol, O: 16.0 g/mol)
(b) An unknown mass of Na3PO4(s) is dissolved in water to form 50.00 mL of solution. This is Solution A. Then 10.00 mL of Solution A is diluted with water to 50.00 mL. The final solution is Solution B. 20.00 mL of Solution B contains 4.408 x 1020 sodium ions. (NA = 6.022 x 1023 mol-1) Calculate the mass of Na3PO4(s) that was dissolved to form Solution A.
Calculate the mass of silver bromide produced from 23.2 g of magnesium bromide in the following reaction: 2AGNO;(aq) + MgBr,(aq) - 2AgBr(s) + Mg(NO)2(aq)
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Balance the following equations. (Use the lowest possible integer coefficients.) (a) UO₂ (s) + HF() → UF4 (s) + H₂O(l) UO₂ (s) + 4 HF () →> (b) B2O3(s) + HF() → BF3 (s) + H₂O(l) B₂O3(s) + HF (1) - (c) BF3 (s) + H₂O(l) → HF() + H3 BO3(s) BF3 (s) + H₂O(l) →→→→ 2 UF4 (s) + BF3 (s) + HF () + 2 H₂O(l) H₂O(l) H3 BO3(s)
Lead (II) carbonate, also called "white lead," was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer be used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is Pb(C₂H3O2)2 (aq) + H₂O(l) + CO₂(g) PbCO3(s) + HC₂H3 O2 (aq) Suppose an aqueous solution containing 1.15 g of lead (II) acetate is treated with 5.80 g of carbon dioxide. Calculate the theoretical yield of lead carbonate. Theoretical yield = g PbCO3
Aqueous solutions of ammonia 1NH32 and bleach (active ingredient NaOCl) are sold as cleaning fluids, but bottles of both of them warn: “Never mix ammonia and bleach, as toxic gases may be produced.” One of the toxic gases that can be produced is chloroamine, NH2Cl.What is the oxidation number of chlorine in chloramine?
6) Consider the following reaction:4NH3 + 50, → 4NO + 6H2O The element being oxidized and the oxidizing agent are: (a)H and NH; (b) O and NH; (c)O and O2 (d) N and O2 (e)N and NH3