Question 1

A limiting reactant is completely consumed in the course of a reaction and may be used to determine how much product may be produced.

Accepted Answer

A limiting reactant is the substance that is entirely used up first in a chemical reaction, thus determining the maximum amount of product that can be formed.

Question 2

Consider the following reaction: 4C + S₈→ 4CS₂. How much S₈ is required for the formation of 6.75 moles of CS₂?

Accepted Answer

C

Question 3

If an 88.2 g charcoal briquette (assume pure carbon)is burned in an unlimited amount of oxygen, what mass of CO₂is produced by the reaction?

Accepted Answer

B

Question 4

Consider the following reaction: CH₄+ 2O₂→ CO₂+ 2H₂O. How much carbon dioxide is produced in the complete combustion of 100.0 g of methane (CH₄)?

Accepted Answer

100.0 g of methane (CH₄) is 100.0 g / 16.04 g/mol = 6.23 mol. According to the stoichiometry of the reaction, 1 mol of CH₄ produces 1 mol of CO₂. Therefore, 6.23 mol of CH₄ will produce 6.23 mol of CO₂.

Question 5

Consider the following reaction: Cl₂O₅+ H₂O → 2HClO₃. How much HClO₃ is produced from 2.5 moles of Cl₂O₅reacting with excess water?

Accepted Answer

The balanced chemical equation shows that 1 mole of Cl₂O₅ produces 2 moles of HClO₃. Therefore, 2.5 moles of Cl₂O₅ will produce 2.5 * 2 = 5.0 moles of HClO₃.

Question 6

Consider this chemical reaction: NaClO( aq )+ HCl( aq )→ NaCl( aq )+ HClO( aq ). How many mL of 6.00 M HCl is required to neutralize 25.00 mL of 2.35 M NaClO?

Accepted Answer

The reaction is a 1:1 molar ratio. Moles of NaClO = 25.00 mL * 2.35 M = 0.05875 moles. Moles of HCl needed = 0.05875 moles. Volume of HCl = 0.05875 moles / 6.00 M = 0.00979 L = 9.79 mL.

Question 7

Nitroglycerin detonates according to the following balanced reaction: 4C₃H₅N₃O₉( l ) → 12CO₂( g )+ 6N₂( g )+ O₂( g )+ 10H₂O( g ). If 1.00 kg of nitroglycerin is detonated, how many liters of products (assume all gases at standard temperature and pressure, so 1.00 mole = 22.4 L of volume)are released?

Accepted Answer

1.00 kg of nitroglycerin is equivalent to 1000 g. The molar mass of nitroglycerin (C₃H₅N₃O₉) is approximately 227 g/mol. Therefore, 1000 g corresponds to about 4.41 moles of nitroglycerin. According to the balanced equation, 4 moles of nitroglycerin produce 29 moles of gas. Thus, 4.41 moles of nitroglycerin will produce approximately 31.96 moles of gas. At STP, 1 mole of gas occupies 22.4 L, so 31.96 moles of gas will occupy about 715 L.

Question 8

The presence of oxygenates such as MTBE in gasoline result in a more complete combustion and reduced unwanted emissions.

Accepted Answer

Oxygenates like MTBE in gasoline can provide additional oxygen during combustion which can lead to more complete combustion and reduced emissions of harmful pollutants. However, there are also concerns about the potential health and environmental impacts of MTBE and other oxygenates.

Question 9

Complete combustion of gasoline will yield carbon dioxide and water as the major products.

Accepted Answer

Complete combustion of gasoline, which is primarily composed of hydrocarbons, results in carbon dioxide and water as the major products when there is sufficient oxygen.

Question 10

Zinc reacts with oxygen to form ZnO. How many moles of ZnO can form from a reaction of 4.43 moles of Zn and 3.05 moles of oxygen?

Accepted Answer

The balanced chemical equation for the reaction is 2Zn + O2 → 2ZnO. This means 2 moles of Zn react with 1 mole of O2 to produce 2 moles of ZnO. With 4.43 moles of Zn, the limiting reactant is Zn, and it will produce 4.43 moles of ZnO.

Question 11

The following reaction illustrates the reaction of methanol with oxygen to form carbon dioxide and water: 2CH₃OH( l )+ 3O₂( g )→ 2CO₂( g )+ 4H₂O( l ). How many moles of water are produced in a reaction of 15 moles of methanol with 30 moles of oxygen?

Accepted Answer

The answer of The following reaction illustrates the reaction of...

Question 12

How many moles of aluminum oxide can form if 26.2 moles of Al metal react with an unlimited amount of oxygen?

Accepted Answer

The balanced chemical equation for the reaction is 4Al + 3O2 → 2Al2O3. From the equation, 4 moles of Al produce 2 moles of Al2O3. Therefore, 26.2 moles of Al will produce (26.2 moles Al * 2 moles Al2O3 / 4 moles Al) = 13.1 moles of Al2O3.

Question 13

Consider this chemical reaction: Sn + NaOH → Na ₂SnO ₂+ H ₂. How many moles of hydrogen are liberated from the complete reaction of 3.47 × 10 ⁴kg of tin metal in excess sodium hydroxide?

Accepted Answer

The molar mass of tin (Sn) is approximately 118.71 g/mol. First, convert the mass of tin to moles: 3.47 × 10^4 kg = 3.47 × 10^7 g. Moles of Sn = 3.47 × 10^7 g / 118.71 g/mol ≈ 2.92 × 10^5 moles. The balanced reaction shows a 1:1 ratio between Sn and H2, so 2.92 × 10^5 moles of hydrogen are liberated.

Question 14

In alkanes, carbon atoms are linked with each other by single bonds.

Accepted Answer

Alkanes are saturated hydrocarbons where carbon atoms are connected by single covalent bonds, following the general formula CnH2n+2.

Question 15

Consider the following reaction: 3NO₂( g )+ H₂O( l ) → 2HNO₃( aq )+ NO( g ). What quantity (L)of NO₂is required to completely react with 125 g of water? Assume that the gases are at standard temperature and pressure; hence, 1.00 mole occupies 22.4 L of volume.

Accepted Answer

To find the volume of NO₂ required, first calculate the moles of H₂O: 125 g H₂O × (1 mol/18.02 g) = 6.94 mol H₂O. According to the balanced equation, 3 moles of NO₂ react with 1 mole of H₂O. Therefore, 6.94 mol H₂O requires 3 × 6.94 = 20.82 mol NO₂. At STP, 1 mole of gas occupies 22.4 L, so 20.82 mol NO₂ × 22.4 L/mol = 466.37 L, which rounds to 466 L.

Question 16

Methane is the major component by weight in gasoline.

Accepted Answer

Gasoline is primarily composed of hydrocarbons in the C4 to C12 range, such as octane, not methane. Methane is a major component of natural gas, not gasoline.

Question 17

An SUV features a 60 L gas tank. Assuming complete combustion and a molecular formula of C ₈H ₁₈for gasoline, approximately what amount of oxygen is consumed per tank of gasoline. Assume a density of 0.78 g\mL for gasoline.

Accepted Answer

The answer of An SUV features a 60 L gas...

Question 18

Sulfuric acid can be manufactured using the following reaction: 2S( s )+ 3O₂( g )+ 2H₂O( l )→ 2H₂SO₄( aq ). If a manufacturing site consumes 65 metric tons (1 metric ton = 1000 kg)of sulfur with unlimited access to O₂and H₂O, how many metric tons of sulfuric acid may be produced?

Accepted Answer

The answer of Sulfuric acid can be manufactured using the...

Question 19

Consider the reaction between NaCl and AgNO₃to form silver chloride. How much of the insoluble precipitate will be recovered if 582.4 g of AgNO₃reacts with excess NaCl?

Accepted Answer

The answer of Consider the reaction between NaCl and AgNO₃to...

Question 20

If 4.21 × 10^{− 3}moles of Ca²⁺react with excess PO₄^{3 −}to form calcium phosphate, how many moles of the solid can form?

Accepted Answer

The balanced chemical equation for the formation of calcium phosphate is 3Ca²⁺ + 2PO₄³⁻ → Ca₃(PO₄)₂. Thus, 3 moles of Ca²⁺ produce 1 mole of Ca₃(PO₄)₂. Therefore, 4.21 × 10⁻³ moles of Ca²⁺ will produce (4.21 × 10⁻³ moles) / 3 = 1.40 × 10⁻³ moles of Ca₃(PO₄)₂.

Quiz 4: Stoichiometry

A limiting reactant is completely consumed in the course of a reaction and may be used to determine how much product may be produced.

Consider the following reaction: 4C + S₈→ 4CS₂. How much S₈ is required for the formation of 6.75 moles of CS₂?

If an 88.2 g charcoal briquette (assume pure carbon) is burned in an unlimited amount of oxygen, what mass of CO₂is produced by the reaction?

Consider the following reaction: CH₄+ 2O₂→ CO₂+ 2H₂O. How much carbon dioxide is produced in the complete combustion of 100.0 g of methane (CH₄) ?

Consider the following reaction: Cl₂O₅+ H₂O → 2HClO₃. How much HClO₃ is produced from 2.5 moles of Cl₂O₅reacting with excess water?

Consider this chemical reaction: NaClO( aq ) + HCl( aq ) → NaCl( aq ) + HClO( aq ) . How many mL of 6.00 M HCl is required to neutralize 25.00 mL of 2.35 M NaClO?

The presence of oxygenates such as MTBE in gasoline result in a more complete combustion and reduced unwanted emissions.

Complete combustion of gasoline will yield carbon dioxide and water as the major products.

Zinc reacts with oxygen to form ZnO. How many moles of ZnO can form from a reaction of 4.43 moles of Zn and 3.05 moles of oxygen?

The following reaction illustrates the reaction of methanol with oxygen to form carbon dioxide and water: 2CH₃OH( l ) + 3O₂( g ) → 2CO₂( g ) + 4H₂O( l ) . How many moles of water are produced in a reaction of 15 moles of methanol with 30 moles of oxygen?

How many moles of aluminum oxide can form if 26.2 moles of Al metal react with an unlimited amount of oxygen?

Consider this chemical reaction: Sn + NaOH → Na ₂SnO ₂+ H ₂. How many moles of hydrogen are liberated from the complete reaction of 3.47 × 10 ⁴kg of tin metal in excess sodium hydroxide?

In alkanes, carbon atoms are linked with each other by single bonds.

Consider the following reaction: 3NO₂( g ) + H₂O( l ) → 2HNO₃( aq ) + NO( g ) . What quantity (L) of NO₂is required to completely react with 125 g of water? Assume that the gases are at standard temperature and pressure; hence, 1.00 mole occupies 22.4 L of volume.

Methane is the major component by weight in gasoline.

An SUV features a 60 L gas tank. Assuming complete combustion and a molecular formula of C ₈H ₁₈for gasoline, approximately what amount of oxygen is consumed per tank of gasoline. Assume a density of 0.78 g\mL for gasoline.

Sulfuric acid can be manufactured using the following reaction: 2S( s ) + 3O₂( g ) + 2H₂O( l ) → 2H₂SO₄( aq ) . If a manufacturing site consumes 65 metric tons (1 metric ton = 1000 kg) of sulfur with unlimited access to O₂and H₂O, how many metric tons of sulfuric acid may be produced?

Consider the reaction between NaCl and AgNO₃to form silver chloride. How much of the insoluble precipitate will be recovered if 582.4 g of AgNO₃reacts with excess NaCl?

If 4.21 × 10^{− 3}moles of Ca²⁺react with excess PO₄^{3 −}to form calcium phosphate, how many moles of the solid can form?

Quiz 4: Stoichiometry

A limiting reactant is completely consumed in the course of a reaction and may be used to determine how much product may be produced.

Consider the following reaction: 4C + S8→ 4CS2. How much S8 is required for the formation of 6.75 moles of CS2?

If an 88.2 g charcoal briquette (assume pure carbon) is burned in an unlimited amount of oxygen, what mass of CO2is produced by the reaction?

Consider the following reaction: CH4+ 2O2→ CO2+ 2H2O. How much carbon dioxide is produced in the complete combustion of 100.0 g of methane (CH4) ?

Consider the following reaction: Cl2O5+ H2O → 2HClO3. How much HClO3 is produced from 2.5 moles of Cl2O5reacting with excess water?

Consider this chemical reaction: NaClO( aq ) + HCl( aq ) → NaCl( aq ) + HClO( aq ) . How many mL of 6.00 M HCl is required to neutralize 25.00 mL of 2.35 M NaClO?

The presence of oxygenates such as MTBE in gasoline result in a more complete combustion and reduced unwanted emissions.

Complete combustion of gasoline will yield carbon dioxide and water as the major products.

Zinc reacts with oxygen to form ZnO. How many moles of ZnO can form from a reaction of 4.43 moles of Zn and 3.05 moles of oxygen?

The following reaction illustrates the reaction of methanol with oxygen to form carbon dioxide and water: ​ 2CH3OH( l ) + 3O2( g ) → 2CO2( g ) + 4H2O( l ) . ​ How many moles of water are produced in a reaction of 15 moles of methanol with 30 moles of oxygen?

How many moles of aluminum oxide can form if 26.2 moles of Al metal react with an unlimited amount of oxygen?

Consider this chemical reaction: Sn + NaOH → Na 2 SnO 2 + H 2 . How many moles of hydrogen are liberated from the complete reaction of 3.47 × 10 4 kg of tin metal in excess sodium hydroxide?

In alkanes, carbon atoms are linked with each other by single bonds.

Consider the following reaction: 3NO2( g ) + H2O( l ) → 2HNO3( aq ) + NO( g ) . What quantity (L) of NO2is required to completely react with 125 g of water? Assume that the gases are at standard temperature and pressure; hence, 1.00 mole occupies 22.4 L of volume.

Methane is the major component by weight in gasoline.

An SUV features a 60 L gas tank. Assuming complete combustion and a molecular formula of C 8 H 18 for gasoline, approximately what amount of oxygen is consumed per tank of gasoline. Assume a density of 0.78 g\mL for gasoline.

Sulfuric acid can be manufactured using the following reaction: ​ 2S( s ) + 3O2( g ) + 2H2O( l ) → 2H2SO4( aq ) . ​ If a manufacturing site consumes 65 metric tons (1 metric ton = 1000 kg) of sulfur with unlimited access to O2and H2O, how many metric tons of sulfuric acid may be produced?

Consider the reaction between NaCl and AgNO3to form silver chloride. How much of the insoluble precipitate will be recovered if 582.4 g of AgNO3reacts with excess NaCl?

If 4.21 × 10 − 3moles of Ca2+react with excess PO43 − to form calcium phosphate, how many moles of the solid can form?

Consider the following reaction: 4C + S₈→ 4CS₂. How much S₈ is required for the formation of 6.75 moles of CS₂?

If an 88.2 g charcoal briquette (assume pure carbon) is burned in an unlimited amount of oxygen, what mass of CO₂is produced by the reaction?

Consider the following reaction: CH₄+ 2O₂→ CO₂+ 2H₂O. How much carbon dioxide is produced in the complete combustion of 100.0 g of methane (CH₄) ?

Consider the following reaction: Cl₂O₅+ H₂O → 2HClO₃. How much HClO₃ is produced from 2.5 moles of Cl₂O₅reacting with excess water?

The following reaction illustrates the reaction of methanol with oxygen to form carbon dioxide and water: 2CH₃OH( l ) + 3O₂( g ) → 2CO₂( g ) + 4H₂O( l ) . How many moles of water are produced in a reaction of 15 moles of methanol with 30 moles of oxygen?

Consider this chemical reaction: Sn + NaOH → Na ₂SnO ₂+ H ₂. How many moles of hydrogen are liberated from the complete reaction of 3.47 × 10 ⁴kg of tin metal in excess sodium hydroxide?

Consider the following reaction: 3NO₂( g ) + H₂O( l ) → 2HNO₃( aq ) + NO( g ) . What quantity (L) of NO₂is required to completely react with 125 g of water? Assume that the gases are at standard temperature and pressure; hence, 1.00 mole occupies 22.4 L of volume.

An SUV features a 60 L gas tank. Assuming complete combustion and a molecular formula of C ₈H ₁₈for gasoline, approximately what amount of oxygen is consumed per tank of gasoline. Assume a density of 0.78 g\mL for gasoline.

Sulfuric acid can be manufactured using the following reaction: 2S( s ) + 3O₂( g ) + 2H₂O( l ) → 2H₂SO₄( aq ) . If a manufacturing site consumes 65 metric tons (1 metric ton = 1000 kg) of sulfur with unlimited access to O₂and H₂O, how many metric tons of sulfuric acid may be produced?

Consider the reaction between NaCl and AgNO₃to form silver chloride. How much of the insoluble precipitate will be recovered if 582.4 g of AgNO₃reacts with excess NaCl?

If 4.21 × 10^{− 3}moles of Ca²⁺react with excess PO₄^{3 −}to form calcium phosphate, how many moles of the solid can form?