Question 1

What is the theoretical yield of PI₃ from the reaction of 27.0 g of P and 68.0 g of I₂? 2P(s)+ 3I₂(s)$\rarr$2PI₃(s)

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Question 2

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory.At times it can be easier to chemically prepare occasionally used gases..For example, nitrogen monoxide, NO(g), can be prepared in the lab using the following chemical reaction: 3Cu(s)+ 8HNO₃(aq)$\rarr$2NO(g)+ 3Cu(NO₃)₂(aq)+ 4H₂O(l) If 5.0 g of copper metal was added to an aqueous solution containing 2.5 moles of HNO₃, how many moles of NO(g)would be produced, assuming a 100% yield.

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Question 3

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC₂(s)+ H₂O(l)$\rarr$HCCH(g)+ CaO(s) How many grams of CaC₂ would be required to generate 0.20 moles of HCCH(g)?

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Question 4

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory.At times, it can be easier to chemically prepare occasionally used gases..For example, oxygen gas can be prepared by heating KMnO₄(s)according to the following chemical reaction: 2KMnO₄(s)$\rarr$ K₂MnO₄(s)+ MnO₂(s)+ O₂(g) How many grams of KMnO₄ would you need to produce 0.27 moles of O₂, assuming 100% conversion? The molar mass of KMnO₄ is 158.034 g/mol.

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Question 5

Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the following reaction: NH₄NO₃ $\rarr$ N₂O + 2H₂O If a 108 g sample of NH₄NO₃ decomposes to give 23 g of N₂O(g), what percent of the original sample remains?

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Question 6

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced.What is the empirical formula of the compound?

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Question 7

Ferrocene, Fe(C₅H₅)₂(s), can be prepared by reacting 3.0 g of FeCl₂(s)with an equal mass of cyclopentadiene, C₅H₆(l), and an excess of KOH, as shown in the following reaction FeCl₂ + 2C₅H₆ + 2KOH $\rarr$ FeC₁₀H₁₀ + 2H₂O A.What is the limiting reagent in this procedure? B.Based on your answer to part A, what mass of Fe(C₅H₅)₂ could theoretically be formed? C.A student who carried out this reaction obtained 2.7 g of ferrocene.What was the percent yield for this reaction?

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Question 8

Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen.The product that was purified and sent off for elemental analysis giving the following mass percents: 68.85% C and 4.95% H.Determine the empirical formula of this compound.

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Question 9

In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia.How many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen, and how many kilograms of ammonia would be formed?

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Question 10

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory.At times, it can be easier to chemically prepare occasionally used gases..For example, nitrogen monoxide, NO(g), can be prepared in the lab by the following chemical reaction: 3Cu(s)+ 8HNO₃(aq)$\rarr$2NO(g)+ 3Cu(NO₃)₂(aq)+ 4H₂O(l) If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO₃, how many moles of NO(g)would be produced, assuming a 75% yield.

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Question 11

The percent composition by mass of tartaric acid is: 32.01% C, 4.03% H, and 63.96% O.Given that the molecular mass of tartaric acid is 150 amu, determine its molecular formula.

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Question 12

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced.What is the empirical formula of the compound?

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Question 13

Determine the number of moles of water produced by the reaction of 155 g of ammonia and 356 g of oxygen. 4NH₃ + 5O₂ $\rarr$4NO + 6H₂O

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Question 14

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory.At times, it can be easier to chemically prepare occasionally used gases..For example, oxygen gas can be prepared by heating KMnO₄(s)according to the following chemical reaction: 2KMnO₄(s)$\rarr$K₂MnO₄(s)+ MnO₂(s)+ O₂(g) The above procedure was carried out starting with 93.2 g of KMnO₄, and it was later determined that all of the KMnO₄ reacted according to the above equation except 11.7 g.What was the percent yield for the reaction?

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Quiz 3: Mass Relationships in Chemical Reactions

What is the theoretical yield of PI₃ from the reaction of 27.0 g of P and 68.0 g of I₂? 2P(s)+ 3I₂(s) $\rarr$ 2PI₃(s)

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC₂(s)+ H₂O(l) $\rarr$ HCCH(g)+ CaO(s) How many grams of CaC₂ would be required to generate 0.20 moles of HCCH(g)?

Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the following reaction: NH₄NO₃ $\rarr$ N₂O + 2H₂O If a 108 g sample of NH₄NO₃ decomposes to give 23 g of N₂O(g), what percent of the original sample remains?

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced.What is the empirical formula of the compound?

Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen.The product that was purified and sent off for elemental analysis giving the following mass percents: 68.85% C and 4.95% H.Determine the empirical formula of this compound.

In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia.How many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen, and how many kilograms of ammonia would be formed?

The percent composition by mass of tartaric acid is: 32.01% C, 4.03% H, and 63.96% O.Given that the molecular mass of tartaric acid is 150 amu, determine its molecular formula.

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced.What is the empirical formula of the compound?

Determine the number of moles of water produced by the reaction of 155 g of ammonia and 356 g of oxygen. 4NH₃ + 5O₂ $\rarr$ 4NO + 6H₂O

Quiz 3: Mass Relationships in Chemical Reactions

What is the theoretical yield of PI3 from the reaction of 27.0 g of P and 68.0 g of I2? 2P(s)+ 3I2(s) →\rarr→ 2PI3(s)

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC2(s)+ H2O(l) →\rarr→ HCCH(g)+ CaO(s) How many grams of CaC2 would be required to generate 0.20 moles of HCCH(g)?

Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the following reaction: NH4NO3 →\rarr→ N2O + 2H2O If a 108 g sample of NH4NO3 decomposes to give 23 g of N2O(g), what percent of the original sample remains?

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO2 and 1.01 g of H2O were produced.What is the empirical formula of the compound?

Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen.The product that was purified and sent off for elemental analysis giving the following mass percents: 68.85% C and 4.95% H.Determine the empirical formula of this compound.

In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia.How many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen, and how many kilograms of ammonia would be formed?

The percent composition by mass of tartaric acid is: 32.01% C, 4.03% H, and 63.96% O.Given that the molecular mass of tartaric acid is 150 amu, determine its molecular formula.

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO2 and 0.826 g of H2O are produced.What is the empirical formula of the compound?

Determine the number of moles of water produced by the reaction of 155 g of ammonia and 356 g of oxygen. 4NH3 + 5O2 →\rarr→ 4NO + 6H2O

What is the theoretical yield of PI₃ from the reaction of 27.0 g of P and 68.0 g of I₂? 2P(s)+ 3I₂(s) $\rarr$ 2PI₃(s)

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC₂(s)+ H₂O(l) $\rarr$ HCCH(g)+ CaO(s) How many grams of CaC₂ would be required to generate 0.20 moles of HCCH(g)?

Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the following reaction: NH₄NO₃ $\rarr$ N₂O + 2H₂O If a 108 g sample of NH₄NO₃ decomposes to give 23 g of N₂O(g), what percent of the original sample remains?

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced.What is the empirical formula of the compound?

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced.What is the empirical formula of the compound?

Determine the number of moles of water produced by the reaction of 155 g of ammonia and 356 g of oxygen. 4NH₃ + 5O₂ $\rarr$ 4NO + 6H₂O