ACTIVITY 1: MASS RELATIONSHIPS IN CHEMICAL REACTIONSDIRECTIONS: Answer the following problems. Write your complete solution on a separate sheet of paper.The combustion of carbon monoxide gas in oxygen gas is represented by the following balanced equation: 2 CO(g) + O2(g) 2 CO2(g)How many moles of carbon dioxide gas will be produced from the complete combustion of 4.60 moles CO(g)? 2. Consider the reaction: 2 KClO32 KCl + 3 O2 How many moles of KClO3are required to produce 22.8 moles of oxygen gas, O2?How many moles of KCl will be produced from the total decomposition of 18.8 moles KClO3? 3. Silver metal reacts with sulfur sulfide according to the following reaction: 2 Ag (s) + S(s) → Ag2S(s)Identify the reagent if 50.0 g Ag reacts with 10.0 g S.What is the theoretical yield in g of Ag2S produced from the reaction?What is the amount in g of the excess reactant expected to remain after the reaction?When the reaction occurred, the amount of Ag2S obtained was 45.0 g. What is the percent yield of the reaction?

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Answered: The combustion of carbon monoxide gas…

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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ACTIVITY 1: MASS RELATIONSHIPS IN CHEMICAL REACTIONS

DIRECTIONS: Answer the following problems. Write your complete solution on a separate sheet of paper.

The combustion of carbon monoxide gas in oxygen gas is represented by the following balanced equation: 2 CO(g) + O₂(g) 2 CO₂(g)

How many moles of carbon dioxide gas will be produced from the complete combustion of 4.60 moles CO(g)?

2. Consider the reaction: 2 KClO₃2 KCl + 3 O₂

How many moles of KClO₃are required to produce 22.8 moles of oxygen gas, O₂?
How many moles of KCl will be produced from the total decomposition of 18.8 moles KClO₃?

3. Silver metal reacts with sulfur sulfide according to the following reaction: 2 Ag (s) + S(s) → Ag₂S(s)

Identify the reagent if 50.0 g Ag reacts with 10.0 g S.

What is the theoretical yield in g of Ag₂S produced from the reaction?

What is the amount in g of the excess reactant expected to remain after the reaction?

When the reaction occurred, the amount of Ag₂S obtained was 45.0 g. What is the percent yield of the reaction?

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