Question 1

In 0.20 mole of phosphoric acid, H3PO4
a. how many H atoms are there?
b. what is the total number of atoms?
c. how many moles of O atoms are there?

Accepted Answer

a. 3.61 × 10²³ H atoms...

Question 2

Calculate the molar mass of rubidium carbonate, Rb2CO3.

Accepted Answer

A)   340.43 g/mol
B)   255.00 g/mol
C)   230.94 g/mol
D)   145.47 g/mol
E)   113.48 g/molF) All of the above
G) B) and E)

Question 3

For a sample consisting of 2.50 g of methane, CH4, calculate
a. the number of moles of methane present.
b. the total number of atoms present.

Accepted Answer

a. 0.156 m...

Question 4

Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. What is its empirical formula?

Accepted Answer

A)   C2H3O4
B)   C3H4O2
C)   C4H3O2
D)   C5H12O4
E)   C2H2OF) B) and C)
G) A) and B)

Question 5

In combustion analysis, the carbon and hydrogen contents of a substance are determined from the CO2 and H2O, respectively, which are collected in the absorbers.

Accepted Answer

A) True 
 B)False

Question 6

Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula?

Accepted Answer

A)   H2N7O8Cl18
B)   H2N2O2Cl
C)   HN3O4Cl9
D)   H4NOCl
E)   H4NOCl2F) B) and D)
G) B) and C)

Question 7

In combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO2 and H2O collected in the absorbers.

Accepted Answer

A) True 
 B)False

Question 8

Potassium dichromate, K2Cr2O7, is used in tanning leather, decorating porcelain, and water proofing fabrics. Calculate the number of chromium atoms in 78.82 g of K2Cr2O7.

Accepted Answer

A)   9.490 × 1025 Cr atoms
B)   2.248 × 1024 Cr atoms
C)   1.124 × 1024 Cr atoms
D)   3.227 × 1023 Cr atoms
E)   1.613 × 1023 Cr atomsF) D) and E)
G) A) and C)

Question 9

Lead(II)  sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II)  sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II)  sulfide?

Accepted Answer

A)   151 g
B)   123 g
C)   50.3 g
D)   37.7 g
E)   9.41 gF) B) and C)
G) None of the above

Question 10

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. 
N2(g)  + 3H2(g)   2NH3(g) 
How many grams of nitrogen are needed to produce 325 grams of ammonia?

Accepted Answer

A)   1070 g
B)   535 g
C)   267 g
D)   178 g
E)   108 gF) B) and C)
G) All of the above

Question 11

Gaseous methanol (CH4O) reacts with oxygen gas to produce carbon dioxide gas and liquid water. Write a balanced equation for this process.

Accepted Answer

2CH₄O(g) + ...

Question 12

Balance the following equation for the combustion of butane, a hydrocarbon used in gas lighters:
C4H10(g) + O2(g) F1F1F1S1F1F1F10 CO2(g) + H2O(l)

Accepted Answer

2C₄H₁₀(g) + 1...

Question 13

Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH) 2.

Accepted Answer

A)   3.28 mol
B)   2.32 mol
C)   0.431 mol
D)   0.305 mol
E)   0.200 molF) C) and E)
G) A) and B)

Question 14

Magnesium (used in the manufacture of light alloys)  reacts with iron(III)  chloride to form magnesium chloride and iron. 3Mg(s)  + 2FeCl3(s)   3MgCl2(s)  + 2Fe(s) 
A mixture of 41.0 g of magnesium ( 3(s)   3MgCl2(s)  + 2Fe(s)  A mixture of 41.0 g of magnesium (   = 24.31 g/mol)  and 175 g of iron(III)  chloride (   = 162.2 g/mol)  is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. A)  Limiting reactant is Mg; 67 g of FeCl3 remain. B)  Limiting reactant is Mg; 134 g of FeCl3 remain. C)  Limiting reactant is Mg; 104 g of FeCl3 remain. D)  Limiting reactant is FeCl3; 2 g of Mg remain. E)  Limiting reactant is FeCl3; 87 g of Mg remain." class="answers-bank-image d-inline" rel="preload" > = 24.31 g/mol)  and 175 g of iron(III)  chloride ( 3(s)   3MgCl2(s)  + 2Fe(s)  A mixture of 41.0 g of magnesium (   = 24.31 g/mol)  and 175 g of iron(III)  chloride (   = 162.2 g/mol)  is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. A)  Limiting reactant is Mg; 67 g of FeCl3 remain. B)  Limiting reactant is Mg; 134 g of FeCl3 remain. C)  Limiting reactant is Mg; 104 g of FeCl3 remain. D)  Limiting reactant is FeCl3; 2 g of Mg remain. E)  Limiting reactant is FeCl3; 87 g of Mg remain." class="answers-bank-image d-inline" rel="preload" > = 162.2 g/mol)  is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

Accepted Answer

A)   Limiting reactant is Mg; 67 g of FeCl3 remain.
B)   Limiting reactant is Mg; 134 g of FeCl3 remain.
C)   Limiting reactant is Mg; 104 g of FeCl3 remain.
D)   Limiting reactant is FeCl3; 2 g of Mg remain.
E)   Limiting reactant is FeCl3; 87 g of Mg remain.F) B) and E)
G) D) and E)

Question 15

What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

Accepted Answer

A)   4.00 × 102 g
B)   25.0 g
C)   17.0 g
D)   4.00 × 10-2 g
E)   2.50 × 10-3 gF) A) and B)
G) A) and C)

Question 16

How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH3? 4NH3(g)  + 5O2(g)   4NO(g)  + 6H2O(g)

Accepted Answer

A)   469.7 g
B)   300.6 g
C)   250.0 g
D)   3.406 g
E)   2.180 gF) A) and E)
G) A) and D)

Question 17

A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8 g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?

Accepted Answer

A)   2.0 × 1022
B)   2.2 × 1022
C)   5.8 × 1023
D)   1.7 × 1025
E)   1.8 × 1025F) C) and E)
G) All of the above

Question 18

One mole of O2 has a mass of 16.0 g.

Accepted Answer

A) True 
 B)False

Question 19

The insecticide DDT was formerly in widespread use, but now it is severely restricted owing to its adverse environmental effects. It is prepared as follows:
C2HCl3O + 2C6H5Cl F1F1F1S1F1F1F10 C14H9Cl5 + H2O
chloral chlorobenzene DDT
If 10.00 g of chloral were reacted with 10.00 g of chlorobenzene
a. what is the maximum amount (mol) of DDT which could be formed?
b. what is the limiting reagent?
c. what is the % yield, if 12.15 g of DDT is produced?

Accepted Answer

a. 0.0444 mol DDT
b....

Question 20

Ammonia, NH3, is produced industrially from nitrogen and hydrogen as follows:
N2(g) + 3H2(g) F1F1F1S1F1F1F10 2NH3(g)
What mass, of which starting material, will remain when 30.0 g of N2 and 10.0 g of H2 react until the limiting reagent is completely consumed?

Accepted Answer

3.52 g of ...

Exam 3: Stoichiometry of Formulas and Equations

Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?

Correct Answer
verified

In 0.20 mole of phosphoric acid, H₃PO₄ a. how many H atoms are there? b. what is the total number of atoms? c. how many moles of O atoms are there?

Correct Answer
verified
a. 3.61 × 10²³ H atoms...
View Answer

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N₂(g) + 3H₂(g)  2NH₃(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

Correct Answer
verified

Gaseous methanol (CH₄O) reacts with oxygen gas to produce carbon dioxide gas and liquid water. Write a balanced equation for this process.

Correct Answer
verified
2CH₄O(g) + ...
View Answer

In combustion analysis, the carbon and hydrogen contents of a substance are determined from the CO₂ and H₂O, respectively, which are collected in the absorbers.

Correct Answer
verified

What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

Correct Answer
verified

For a sample consisting of 2.50 g of methane, CH₄, calculate a. the number of moles of methane present. b. the total number of atoms present.

Correct Answer
verified
a. 0.156 m...
View Answer

Potassium dichromate, K₂Cr₂O₇, is used in tanning leather, decorating porcelain, and water proofing fabrics. Calculate the number of chromium atoms in 78.82 g of K₂Cr₂O₇.

Correct Answer
verified

In combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO₂ and H₂O collected in the absorbers.

Correct Answer
verified

Correct Answer
verified
a. 0.0444 mol DDT
b....
View Answer

How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH₃? 4NH₃(g) + 5O₂(g)  4NO(g) + 6H₂O(g)

Correct Answer
verified

Balance the following equation for the combustion of butane, a hydrocarbon used in gas lighters: C₄H₁₀(g) + O₂(g)  CO₂(g) + H₂O(l)

Correct Answer
verified
2C₄H₁₀(g) + 1...
View Answer

Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂and 0.226 g H₂O. What is its empirical formula?

Correct Answer
verified

Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula?

Correct Answer
verified

A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8 g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?

Correct Answer
verified

One mole of O₂ has a mass of 16.0 g.

Correct Answer
verified

Calculate the molar mass of rubidium carbonate, Rb₂CO₃.

Correct Answer
verified

Correct Answer
verified

Ammonia, NH₃, is produced industrially from nitrogen and hydrogen as follows: N₂(g) + 3H₂(g)  2NH₃(g) What mass, of which starting material, will remain when 30.0 g of N₂ and 10.0 g of H₂react until the limiting reagent is completely consumed?

Correct Answer
verified
3.52 g of ...
View Answer

Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH) ₂.

Correct Answer
verified

Exam 3: Stoichiometry of Formulas and Equations

Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?

Correct AnswerverifiedShow Answer

In 0.20 mole of phosphoric acid, H3PO4 a. how many H atoms are there? b. what is the total number of atoms? c. how many moles of O atoms are there?

Correct Answerverifieda. 3.61 × 1023 H atoms...View AnswerShow Answer

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N2(g) + 3H2(g)  2NH3(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

Correct AnswerverifiedShow Answer

Gaseous methanol (CH4O) reacts with oxygen gas to produce carbon dioxide gas and liquid water. Write a balanced equation for this process.

Correct Answerverified2CH4O(g) + ...View AnswerShow Answer

In combustion analysis, the carbon and hydrogen contents of a substance are determined from the CO2 and H2O, respectively, which are collected in the absorbers.

Correct AnswerverifiedShow Answer

What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

Correct AnswerverifiedShow Answer

For a sample consisting of 2.50 g of methane, CH4, calculate a. the number of moles of methane present. b. the total number of atoms present.

Correct Answerverifieda. 0.156 m...View AnswerShow Answer

Potassium dichromate, K2Cr2O7, is used in tanning leather, decorating porcelain, and water proofing fabrics. Calculate the number of chromium atoms in 78.82 g of K2Cr2O7.

Correct AnswerverifiedShow Answer

In combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO2 and H2O collected in the absorbers.

Correct AnswerverifiedShow Answer

Correct Answerverifieda. 0.0444 mol DDTb....View AnswerShow Answer

How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH3? 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g)

Correct AnswerverifiedShow Answer

Balance the following equation for the combustion of butane, a hydrocarbon used in gas lighters: C4H10(g) + O2(g)  CO2(g) + H2O(l)

Correct Answerverified2C4H10(g) + 1...View AnswerShow Answer

Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. What is its empirical formula?

Correct AnswerverifiedShow Answer

Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula?

Correct AnswerverifiedShow Answer

A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8 g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?

Correct AnswerverifiedShow Answer

One mole of O2 has a mass of 16.0 g.

Correct AnswerverifiedShow Answer

Calculate the molar mass of rubidium carbonate, Rb2CO3.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Ammonia, NH3, is produced industrially from nitrogen and hydrogen as follows: N2(g) + 3H2(g)  2NH3(g) What mass, of which starting material, will remain when 30.0 g of N2 and 10.0 g of H2 react until the limiting reagent is completely consumed?

Correct Answerverified3.52 g of ...View AnswerShow Answer

Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH) 2.

Correct AnswerverifiedShow Answer

Correct Answer
verified

In 0.20 mole of phosphoric acid, H₃PO₄ a. how many H atoms are there? b. what is the total number of atoms? c. how many moles of O atoms are there?

Correct Answer
verified
a. 3.61 × 10²³ H atoms...
View Answer

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N₂(g) + 3H₂(g)  2NH₃(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

Correct Answer
verified

Gaseous methanol (CH₄O) reacts with oxygen gas to produce carbon dioxide gas and liquid water. Write a balanced equation for this process.

Correct Answer
verified
2CH₄O(g) + ...
View Answer

In combustion analysis, the carbon and hydrogen contents of a substance are determined from the CO₂ and H₂O, respectively, which are collected in the absorbers.

Correct Answer
verified

Correct Answer
verified

For a sample consisting of 2.50 g of methane, CH₄, calculate a. the number of moles of methane present. b. the total number of atoms present.

Correct Answer
verified
a. 0.156 m...
View Answer

Potassium dichromate, K₂Cr₂O₇, is used in tanning leather, decorating porcelain, and water proofing fabrics. Calculate the number of chromium atoms in 78.82 g of K₂Cr₂O₇.

Correct Answer
verified

In combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO₂ and H₂O collected in the absorbers.

Correct Answer
verified

Correct Answer
verified
a. 0.0444 mol DDT
b....
View Answer

How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH₃? 4NH₃(g) + 5O₂(g)  4NO(g) + 6H₂O(g)

Correct Answer
verified

Balance the following equation for the combustion of butane, a hydrocarbon used in gas lighters: C₄H₁₀(g) + O₂(g)  CO₂(g) + H₂O(l)

Correct Answer
verified
2C₄H₁₀(g) + 1...
View Answer

Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂and 0.226 g H₂O. What is its empirical formula?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

One mole of O₂ has a mass of 16.0 g.

Correct Answer
verified

Calculate the molar mass of rubidium carbonate, Rb₂CO₃.

Correct Answer
verified

Correct Answer
verified

Ammonia, NH₃, is produced industrially from nitrogen and hydrogen as follows: N₂(g) + 3H₂(g)  2NH₃(g) What mass, of which starting material, will remain when 30.0 g of N₂ and 10.0 g of H₂react until the limiting reagent is completely consumed?

Correct Answer
verified
3.52 g of ...
View Answer

Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH) ₂.

Correct Answer
verified