#4 pl Stoichiometry Test Study Guide1). 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 bythe 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 sulfurdioxide 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 itwas used as a dye in yellow paint. Lead poisoning could result if you eat the paint so different dye is used in today'spaint.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 is8.67 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 #1CaC2 + H20 → Ca(OH)2 + C2H2System #2Na2B407 +H2SO4 +H20 → H3B03+ Na2S045). Define limiting reactant, excess reactant and percent yield and the law of conservation of mass.

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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 NazB407 +H2SO4 +H20 → H3B03+ Na2S04

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 NazB407 +H2SO4 +H20 → H3B03+ Na2S04

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.81PAE: 3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

#4 pl

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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