**Preparation of Chlorine in the Laboratory**Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation:\[ \text{MnO}_2(s) + 4 \text{HCl}(aq) \rightarrow \text{MnCl}_2(aq) + 2 \text{H}_2\text{O}(l) + \text{Cl}_2(g) \]**Problem**How much \(\text{MnO}_2(s)\) should be added to excess \(\text{HCl}(aq)\) to obtain 395 mL \(\text{Cl}_2(g)\) at 25 °C and 735 Torr?**Input Box**- **mass of \(\text{MnO}_2\):** [Input box] g**Tools and Controls**- There is a section titled "TOOLS" with an option labeled \(x10^y\) for scientific notation entry.

Answered: Image /qna-images/answer/880cff36-eb18-4193-87ce-b1f95bacfd47.jpg

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) MnCl, (aq) + 2 H,O() + Cl, (g) How much MnO, (s) should be added to excess HC1(aq) to obtain 395 mL Cl, (g) at 25 °C and 735 Torr? mass of MnO2: g > TOOLS х10

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) MnCl, (aq) + 2 H,O() + Cl, (g) How much MnO, (s) should be added to excess HC1(aq) to obtain 395 mL Cl, (g) at 25 °C and 735 Torr? mass of MnO2: g > TOOLS х10

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

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
If 16.0 mL of water are added to 31.5 mL of 0.586 M Ba(OH)2Ba(OH)2 (aq), what is the new solution molarity?
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) MnCl, (aq) + 2 H,0(1) + Cl,(g) How much MnO,(s) should be added to excess HCI(aq) to obtain 145 mL Cl, (g) at 25 °C and 735 Torr? 1.097 mass of MnO, : Incorrect
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 HCI(aq) → MnCl,(aq) + 2 H,O(1) + Cl, (g) How much MnO, (s) should be added to excess HCl(aq) to obtain 345 mL Cl, (g) at 25 °C and 765 Torr? mass of MnO,:
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 265 mL Cl2(g) at 25 °C and 735 Torr? mass of MnO2:_________________________________________________
Hw.10.
A 3.27 g sample of iron ore is transformed to a solution of iron(II) sulfate, FeSO4. This solution is titrated with 0.110 M K2CT20, (potassium dichromate). If it requires 58.3 ml of potassium dichromate solution to titrate the iron(II) sulfate solution, what is the percentage of iron in the ore? The reaction is 6FESO, (aq) + K, Cr2O; (aq) + 7H;SO4 (aq) + 3Fe; (SO,)a (aq) + Cr2 (SO4)a (ag) + 7H2O(1) + K2SO, (ag) Percentage =
The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S₂O3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2 S₂O3(aq) + ₂ (aq) → S₂O²(aq) + 31 (aq) Given that it requires 35.5 mL of 0.440 M Na₂S₂O3(aq) to titrate a 30.0 mL sample of I3 (aq), calculate the molarity of I3 (aq) in the solution. [1] = M
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO,(s) + 4 HCI(aq) → MnCl, (aq) + 2 H,O(1) + Cl, (g) How much Mn0,(s) should be added to excess HCI(aq) to obtain 125 mL Cl, (g) at 25 °C and 705 Torr? mass of MnO,: Question Source: McQuarrie, Rock, And Gallogly 4e- General Chemsitry Publisher: University Scienc
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) MnCl, (aq) + 2 H,0(1) + Cl, (g) How much MnO, (s) should be added to excess HCl(aq) to obtain 205 mL CI, (g) at 25 °C and 735 Torr? mass of MnO2: g
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) - MnCl, (aq) + 2 H,O(1) + Cl, (g) How much Mn0, (s) should be added to excess HCI(aq) to obtain 235 mL Cl, (g) at 25 °C and 735 Torr? mass of MnO,: g
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)?