Diarsenic trioxide reacts with water to form arsenous acid (H3AsO3). a. Write a balanced equation for the reaction described above. b. Identify the reaction type (combustion, single replacement, double replacement, synthesis or decomposition) c.For the reaction of 68.8 g of diarsenic trioxidewith 18.8 g water, calculate the theoretical yield of arsenous acid. d. Identify the limiting reactant. e. Calculate how many grams of excess reactant remain at the end of the reaction: f. If 64.4g of arsenous acidare actually formed in the lab, calculate the percent yield for the reaction.
Diarsenic trioxide reacts with water to form arsenous acid (H3AsO3). a. Write a balanced equation for the reaction described above. b. Identify the reaction type (combustion, single replacement, double replacement, synthesis or decomposition) c.For the reaction of 68.8 g of diarsenic trioxidewith 18.8 g water, calculate the theoretical yield of arsenous acid. d. Identify the limiting reactant. e. Calculate how many grams of excess reactant remain at the end of the reaction: f. If 64.4g of arsenous acidare actually formed in the lab, calculate the percent yield for the reaction.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 121QRT: Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A...
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Diarsenic trioxide reacts with water to form arsenous acid (H3AsO3).
a. Write a balanced equation for the reaction described above.
b. Identify the reaction type (combustion, single replacement, double replacement, synthesis or decomposition)
c.For the reaction of 68.8 g of diarsenic trioxidewith 18.8 g water, calculate the theoretical yield of arsenous acid.
d. Identify the limiting reactant.
e. Calculate how many grams of excess reactant remain at the end of the reaction:
f. If 64.4g of arsenous acidare actually formed in the lab, calculate the percent yield for the reaction.
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