A chemist reacts 63.1 g of hydrogen chloride with 17.2 g of oxygen gas. The reaction produces chlorine gas and water. Remember that oxygen and chlorine exist naturally as diatomic molecules. A) Write a balanced chemical equation for this reaction. B) Calculate the theoretical yield of chlorine gas in grams. C) Identify the limiting reactant. D) Calculate the grams of each reactant at the end of the reaction. E) What is the percent yield of the reaction if 49.3 g of chlorine gas is collected after the reaction is complete. _ HCl(g) + _ O2(g) ⟶ _ Cl2(g) + _ H2O(g)
A chemist reacts 63.1 g of hydrogen chloride with 17.2 g of oxygen gas. The reaction produces chlorine gas and water. Remember that oxygen and chlorine exist naturally as diatomic molecules. A) Write a balanced chemical equation for this reaction. B) Calculate the theoretical yield of chlorine gas in grams. C) Identify the limiting reactant. D) Calculate the grams of each reactant at the end of the reaction. E) What is the percent yield of the reaction if 49.3 g of chlorine gas is collected after the reaction is complete. _ HCl(g) + _ O2(g) ⟶ _ Cl2(g) + _ H2O(g)
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 19CR
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A chemist reacts 63.1 g of hydrogen chloride with 17.2 g of oxygen gas. The reaction produces chlorine gas and water. Remember that oxygen and chlorine exist naturally as diatomic molecules. A) Write a balanced chemical equation for this reaction. B) Calculate the theoretical yield of chlorine gas in grams. C) Identify the limiting reactant. D) Calculate the grams of each reactant at the end of the reaction. E) What is the percent yield of the reaction if 49.3 g of chlorine gas is collected after the reaction is complete.
_ HCl(g) + _ O2(g) ⟶ _ Cl2(g) + _ H2O(g)
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