"Nitric acid reacts with S to give H2SO4 and nitrogen monoxide. 30 ml of acid at 25% by mass and a density of 1.08 g/ml with 5 g of S. a) Adjust the reaction. b) Calculate limiting reactant and its excess. c) Calculate mass of unreacted reactant. d) Determine volume of NO at 600 mm Hg and 20°C. 20% yield" THE EQUATION THEY PROVIDE IS: 2HNO3 + S → H2SO4 +2NO YOU DONT NEED TO ADD H20 IN THE EQUATION
"Nitric acid reacts with S to give H2SO4 and nitrogen monoxide. 30 ml of acid at 25% by mass and a density of 1.08 g/ml with 5 g of S. a) Adjust the reaction. b) Calculate limiting reactant and its excess. c) Calculate mass of unreacted reactant. d) Determine volume of NO at 600 mm Hg and 20°C. 20% yield" THE EQUATION THEY PROVIDE IS: 2HNO3 + S → H2SO4 +2NO YOU DONT NEED TO ADD H20 IN THE EQUATION
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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"Nitric acid reacts with S to give H2SO4 and nitrogen monoxide. 30 ml of acid at 25% by mass and a density of 1.08 g/ml with 5 g of S.
a) Adjust the reaction.
b) Calculate limiting reactant and its excess.
c) Calculate mass of unreacted reactant.
d) Determine volume of NO at 600 mm Hg and 20°C. 20% yield"
THE EQUATION THEY PROVIDE IS:
2HNO3 + S → H2SO4 +2NO
YOU DONT NEED TO ADD H20 IN THE EQUATION
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Step 1: Defining the limiting reagent!
VIEWStep 2: Finding out the mass of the solution!
VIEWStep 3: Finding out the number of moles of nitric acid used!
VIEWStep 4: Finding out the number of moles of sulfur used!
VIEWStep 5: Finding out the limiting reagent!
VIEWStep 6: Finding out the actual yield of NO!
VIEWStep 7: Finding out the unreacted mass of nitric acid and sulfur!
VIEWStep 8: Finding out the volume of NO produced!
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