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3.00 g MnO2 are combined with 200.00ml of 2.20 M HCl according to the reaction: _ MnO2 (s) +_ HC1 (ag) → _ Cl2 (g) + _ H;O(1) + _ MnCl2(3g). (Unbalanced equation) (Molar mass of Mn (in g/mol): 55; O:16; H: 1; Cl: 35.5) (a) Give the balanced equation for the above reaction. (b) Name the compound of MnO2. (c) Determine the limiting reactant. Show the calculation steps clearly. (d) Determine the excess amount, in mol, of the other reactant. (e) Calculate the mass of Cl2 produced, given that the % yield is 75%.

3.00 g MnO2 are combined with 200.00ml of 2.20 M HCl according to the reaction: _ MnO2 (s) +_ HC1 (ag) → _ Cl2 (g) + _ H;O(1) + _ MnCl2(3g). (Unbalanced equation) (Molar mass of Mn (in g/mol): 55; O:16; H: 1; Cl: 35.5) (a) Give the balanced equation for the above reaction. (b) Name the compound of MnO2. (c) Determine the limiting reactant. Show the calculation steps clearly. (d) Determine the excess amount, in mol, of the other reactant. (e) Calculate the mass of Cl2 produced, given that the % yield is 75%.

Chemistry
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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3.00 g MnO2 are combined with 200.00ml of 2.20 M HCl according to the reaction: _MnO, (s) +_ HCi (ag) → _ Cl2 (g) + _ H20(1) + _ MnCl,(ag). (Unbalanced equation) (Molar mass of Mn (in g/mol): 55; 0:16; H: 1; Cl: 35.5) (a) Give the balanced equation for the above reaction. (b) Name the compound of MnO,. (c) Determine the limiting reactant. Show the calculation steps clearly. (d) Determine the excess amount, in mol, of the other reactant. (e) Calculate the mass of Cl; produced, given that the % yield is 75%.
Transcribed Image Text:3.00 g MnO2 are combined with 200.00ml of 2.20 M HCl according to the reaction: _MnO, (s) +_ HCi (ag) → _ Cl2 (g) + _ H20(1) + _ MnCl,(ag). (Unbalanced equation) (Molar mass of Mn (in g/mol): 55; 0:16; H: 1; Cl: 35.5) (a) Give the balanced equation for the above reaction. (b) Name the compound of MnO,. (c) Determine the limiting reactant. Show the calculation steps clearly. (d) Determine the excess amount, in mol, of the other reactant. (e) Calculate the mass of Cl; produced, given that the % yield is 75%.
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