Stoichiometry Test Study Guide 1). Laughing gas, N20, can be turned into smog, NO2, by heating the laughing gas in the presence of oxygen: 2N20(g) + 302(g) → 4NO2(g) A) 9.00 grams of laughing gas react. How many moles of oxygen react? B) If 7.50 grams of oxygen react, how many grams of smog are produced? C) If 2.5 moles of smog needs to be created, how many moles of laughing gas are required? D) If 3.00 moles of oxygen creates 3.75 moles of smog, what is the percent yield? 2). Thionyl chloride, SOC12, is used as a powerful drying agent. The thionyl chloride reacts with water as shown by the reaction: SOCI2 (1) + H20(1) → S02(g) + 2HCI(g) A) 35.0 grams of thionyl chloride is placed in a glass containing 500.0 grams of water. How many grams of sulfur dioxide will be created? B) After the reaction is complete how many grams of the excess reactant will remain unreacted? 3). Consider the reaction below. The lead (II) iodide is a bright yellow insoluble substance. Prior to the 1960's it was used as a dye in yellow paint. Lead poisoning could result if you eat the paint so different dye is used in today's paint. A) If 10.0 grams of sodium iodide react, how many grams of lead (II) iodide are produced? _Nal +_Pb(NO3)2 →_NaNO3 +_Pbl2 (Balance first!!!) B) When a student completes this reaction, she filters and dries the lead (II) iodide. The mass of the yellow solid is 8.67 grams. What is the actual, theoretical and percent yield? 4). For each of the unbalanced reactions below 5.00 grams of each reactant is mixed together. A) Balance the reaction. B) Find the mass of the first product made by the reaction. C) Determine which substance is the limiting reactant. D) Determine the mass of each excess reactant that remains after the reaction is complete. System #1 CaC2 + H20 → Ca(OH)2 + C2H2 System #2 Na2B407 +H2SO4 +H20 → H3BO3+ Na2S04 5). Define limiting reactant, excess reactant and percent yield and the law of conservation of mass.
Stoichiometry Test Study Guide 1). Laughing gas, N20, can be turned into smog, NO2, by heating the laughing gas in the presence of oxygen: 2N20(g) + 302(g) → 4NO2(g) A) 9.00 grams of laughing gas react. How many moles of oxygen react? B) If 7.50 grams of oxygen react, how many grams of smog are produced? C) If 2.5 moles of smog needs to be created, how many moles of laughing gas are required? D) If 3.00 moles of oxygen creates 3.75 moles of smog, what is the percent yield? 2). Thionyl chloride, SOC12, is used as a powerful drying agent. The thionyl chloride reacts with water as shown by the reaction: SOCI2 (1) + H20(1) → S02(g) + 2HCI(g) A) 35.0 grams of thionyl chloride is placed in a glass containing 500.0 grams of water. How many grams of sulfur dioxide will be created? B) After the reaction is complete how many grams of the excess reactant will remain unreacted? 3). Consider the reaction below. The lead (II) iodide is a bright yellow insoluble substance. Prior to the 1960's it was used as a dye in yellow paint. Lead poisoning could result if you eat the paint so different dye is used in today's paint. A) If 10.0 grams of sodium iodide react, how many grams of lead (II) iodide are produced? _Nal +_Pb(NO3)2 →_NaNO3 +_Pbl2 (Balance first!!!) B) When a student completes this reaction, she filters and dries the lead (II) iodide. The mass of the yellow solid is 8.67 grams. What is the actual, theoretical and percent yield? 4). For each of the unbalanced reactions below 5.00 grams of each reactant is mixed together. A) Balance the reaction. B) Find the mass of the first product made by the reaction. C) Determine which substance is the limiting reactant. D) Determine the mass of each excess reactant that remains after the reaction is complete. System #1 CaC2 + H20 → Ca(OH)2 + C2H2 System #2 Na2B407 +H2SO4 +H20 → H3BO3+ Na2S04 5). Define limiting reactant, excess reactant and percent yield and the law of conservation of mass.
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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Transcribed Image Text:Stoichiometry Test Study Guide
1). Laughing gas, N20, can be turned into smog, NO2, by heating the laughing gas in the presence of oxygen:
2N20(g) + 302(g) → 4NO2(g)
A) 9.00 grams of laughing gas react. How many moles of oxygen react?
B) If 7.50 grams of oxygen react, how many grams of smog are produced?
C) If 2.5 moles of smog needs to be created, how many moles of laughing gas are required?
D) If 3.00 moles of oxygen creates 3.75 moles of smog, what is the percent yield?
2). Thionyl chloride, SOC12, is used as a powerful drying agent. The thionyl chloride reacts with water as shown by
the reaction: SOCI2 (1) + H20(1) → SO2(g) + 2HCI(g)
A) 35.0 grams of thionyl chloride is placed in a glass containing 500.0 grams of water. How many grams of sulfur
dioxide will be created?
B) After the reaction is complete how many grams of the excess reactant will remain unreacted?
3). Consider the reaction below. The lead (II) iodide is a bright yellow insoluble substance. Prior to the 1960's it
was used as a dye in yellow paint. Lead poisoning could result if you eat the paint so different dye is used in today's
paint.
A) If 10.0 grams of sodium iodide react, how many grams of lead (II) iodide are produced?
_Nal +_Pb(NO3)2 →_NaNO3 +_Pbl2 (Balance first!!!)
B) When a student completes this reaction, she filters and dries the lead (II) iodide. The mass of the yellow solid is
8.67 grams. What is the actual, theoretical and percent yield?
4). For each of the unbalanced reactions below 5.00 grams of each reactant is mixed together.
A) Balance the reaction.
B) Find the mass of the first product made by the reaction.
C) Determine which substance is the limiting reactant.
D) Determine the mass of each excess reactant that remains after the reaction is complete.
System #1
CaC2 + H20 → Ca(OH)2 + C2H2
System #2
Na2B407 +H2SO4 +H20 → H3B03+ Na2S04
5). Define limiting reactant, excess reactant and percent yield and the law of conservation of mass.
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