A 4.510 g rock sample is dissolved in strong acid and treated with a reducing agent so that all the iron iscompletely transformed into Fe2+. The Fe2* is completely oxidized by 28.10 mL of a 0.0530 M solution ofKMNO4. Calculate the amount of iron (in grams) and its mass percentage in the rock sample.MnO4 (ag) + Fe2* (ag)Mn2+ (ag) + Fe3+ (ag)MM: KMNO4 = 158.03Fe = 55.85%3D

In this reaction Fe 2+ oxidised to Fe3+ and MnO4- reduced to Mn2+ . After balance the reaction we…

Answered: A 4.510 g rock sample is dissolved in…

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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A sample of iron ore is dissolved in acid, and the iron is converted to Fe2*. The sample is then titrated with 47.20 mL of 0.02240 M MnO4 solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) → Mn²*(aq) + 5FE3* (aq) + 4H2O How many moles of MnO4¯ were added to the solution? Blank 1 2+ How many moles of Fe were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4 Blank 1 Add your answer Blank 2 Add your answer Blank 3 Add your answer Blank 4 Add your answer
Ca(ClO3)2 (aq) + NH4F (aq) -> CaF2 (s) + ? A.) Determine the product. B.) Balance the equation C.) Write the net ionic reaction D.) Identify the spectator ions
Excess Na2SO4(aq) is added to a 4.41×102 mL sample of industrial waste containing Ba2+ ions. If 55.5 g of BaSO4(s) are precipitated from the reaction, what was the molar concentration of Ba2+ in the original sample?
The quantity of antimony in a sample can be determined by an oxidation–reduction titration with an oxidizing agent. A 6.19 g6.19 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+⁢(aq). The Sb3+⁢(aq) is completely oxidized by 30.5 mL of a 0.115 M aqueous solution of KBrO3⁢(aq). The unbalanced equation for the reaction is BrO^− 3(aq) + Sb^3+(aq)⟶Br^−(aq)+Sb^5+(aq)(unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony in grams: percentage of antimony:
Based on the balanced chemical equation shown below, determine the mass percent of Fest in a 0.5450 g sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with the Fe3+ present in the ore sample. The chemical equation for the reaction is 2 Fe3+(aq) + Sn2+(aq) → 2 Fe2*(aq) + Sn4+(aq). O 22.95% O 7.333% O 11.48% O 45.91%
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
A student investigated the stoichiometry of the reaction of zinc (Zn) with HCI solution and reported the following data: When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCI, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 10 M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol. The density of water at 27.0 °C is 0.9965 g mLand its vapor pressure is 27.0 torr. R = 8.21 X.10 2 L- atm K mol 1 Calculate the number of millimoles of HCI remaining in the flask at the end of the reaction
In the following chemical reaction, which element is the reducing agent? 3 Sn(NO₃)₂(aq) + 2 Fe(s) → 2 Fe(NO₃)₃(aq) + 3 Sn(s)
write the net ionic equation for the reaction in the photo
write the net ionic equation for Cu(s) + 4HNO3(aq) = 2NO2(g) + Cu(NO3)2(aq) + 2H2O(l)

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