Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HC1(aq), as described by the chemical equation MnO,(s) + 4 HC1(aq) MnCl, (aq) + 2 H,O(1) + Cl,(g) How much MnO, (s) should be added to excess HC1(aq) to obtain 175 mL Cl, (g) at 25 °C and 775 Torr? mass of MnO,:

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HC1(aq), as described by the chemical equation MnO,(s) + 4 HC1(aq) MnCl, (aq) + 2 H,O(1) + Cl,(g) How much MnO, (s) should be added to excess HC1(aq) to obtain 175 mL Cl, (g) at 25 °C and 775 Torr? mass of MnO,:

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...

See similar textbooks

Similar questions

A solution of NaCl(aq)NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq)Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.05 g PbCl2(s)10.05 g PbCl2(s) is obtained from 200.0 mL200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq)Pb(NO3)2(aq) solution.
Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(II) to insoluble Fe(III): $$4Fe(OH)+(aq)+4OH−(aq)+O2(g)+2H2O(l)4Fe(OH)3(s) How many grams of O2 are consumed to precipitate all of the iron in 75.0 mL of 0.0350 M Fe(II)?
To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.390M silver nitrate (AgNO,) solution to a 45.0 g sample of the fluid and collects the solid silver chloride (AgCl) product. When no more AgCl is produced, she filters, washes and weighs it, and finds that 1.8 g has been produced. The balanced chemical equation for the reaction is: Cl(aq) + AgNO, (aq) What kind of reaction is this? AgCl(s) + NO, (aq) If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has 2 significant digits. precipitation O acid-base O redox 0 0 0 0% 0° 0 0..9 X 5 A
Suppose you took a 3.00 mL sample of HNO3 (aq) of an unknown concentration, and find that you have to add 20.30 mL of 0.106 M NaOH from your buret to neutralize the acid. How many moles of OH- Ions are neutralized in this reaction?
A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00M NaCl (ag) in an Erlenmeyer flask. Both the AgNO3 (aq) solution and the NaCl(aq) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. What is the expected mass of AgCl (s), in grams, assuming that the yield is 100%? In the box, enter the mass to the nearest gram.
A noncarbonated soft drink contains an unknown amount of citric acid, H3 C6H5 O7. If 100. mL of the soft drink requires 35.96 mL of 0.0115 M NaOH to neutralize the citric acid completely, what mass of citric acid does the soft drink contain per 100. mL? The reaction of citric acid and NaOH is Mass= H3 C6H5O7 (aq) + 3 NaOH(aq) → Na3 C6H5O7 (aq) + 3 H₂O(l) g
Calculate the molarity of an acetic acid solution if 26.0 mL of an HC2H3O2 solution is titrated with 24.8 mL of a 0.169 M KOH solution: HC₂H3O2 (aq) + KOH(aq) → H₂O(1)+ KC₂H3O2 (aq) Express your answer with the appropriate units.
How many grams of Ag₂CO3 will precipitate when excess Na₂CO3 solution is added to 49.0 mL of 0.590 M AgNO3 solution? 2AgNO3(aq) + Na2CO3(aq) → Ag2 CO3(s) + 2NaNO3(aq) g
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 10.67 g PbCl₂ (s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)₂(aq) solution. concentration: M
A lab student dissolves 0.401 g of AgNO3 in a beaker of water and 0.253 g of MgCl2 in another beaker of water. The student then combines the two solutions, which together form AgCl as a white precipitate. He then isolates the AgCl and finds its mass to be 0.292 g. Here is the equation for the reaction: (First balance the reaction, if needed) AgNO3 (aq) + MgCl2 (aq) →AgCl (s) + Mg(NO3)2 Which starting material is the limiting reagent? What is the theoretical yield of AgCl in this reaction? What was the percent yield of AgCl in this reaction?
What quantity in moles of precipitate will be formed when 219.5 mL of 0.350 M NaCl is reacted with excess Pb(NO:)2 in the following chemical reaction? 2 NaCl(aq) + Pb(NO:):(aq) → PbCl:(s) + 2 NaNO:(aq)
Fe(lI) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(ll) to insoluble Fe(lI): 4Fe(OH)*(aq) +40H¯(aq)+O2(g) +2H,0(1) → 4Fe(OH),(s) How many grams of O2 are consumed to precipitate all of the iron in 50.0 mL of 0.0950 MFe(II)?