Question 1

What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s)+ 2 H₂O (l)→ Mg(OH)₂ (s)+ H₂ (g) A)0.102 B)0.0162 C)0.0485 D)0.219 E)0.204

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Question 2

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s)+ 3O₂ (g)→ 2SO₃ (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O₂ produced 0.80 g of SO₃. The % yield in this experiment is __________. A)30 B)29 C)21 D)88 E)48

Accepted Answer

Theoretical yield of SO₃ is calculated based on the limiting reactant, which is O₂. The molar mass of O₂ is 32 g/mol, so 1.0 g O₂ is 0.03125 mol. According to the balanced equation, 3 mol of O₂ produce 2 mol of SO₃, so 0.03125 mol O₂ produces 0.02083 mol SO₃. The molar mass of SO₃ is 80 g/mol, so the theoretical yield is 0.02083 mol × 80 g/mol = 1.6664 g. The percent yield is (0.80 g / 1.6664 g) × 100% = 48%.

Question 3

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s)+ 3 O₂ (g)→ 2 Al₂O₃ (s) The maximum amount of Al₂O₃ that can be produced from 2.5 g of Al and 2.5 g of O₂ is __________ g. A)9.4 B)7.4 C)4.7 D)5.3 E)5.0

Accepted Answer

First, we need to determine the limiting reactant. To do this, we calculate the moles of each reactant using their respective molar masses:
moles of Al = 2.5 g / 26.98 g/mol = 0.093 mol
moles of O2 = 2.5 g / 32 g/mol = 0.078 mol
The stoichiometric ratio of Al to O2 is 4:3. Therefore, we see that O2 is the limiting reactant as there are fewer moles of O2 available to react than Al. 
Next, we use the stoichiometry of the balanced equation to calculate the moles of Al2O3 that can be formed:
moles of Al2O3 = 0.078 mol O2 x (2 mol Al2O3 / 3 mol O2) = 0.052 mol Al2O3
Finally, we convert moles of Al2O3 to grams using its molar mass:
mass of Al2O3 = 0.052 mol x 101.96 g/mol = 5.31 g
Therefore, the maximum amount of Al2O3 that can be produced is 5.31 g. The closest answer choice is C, 4.7 g, which is the correct choice.

Question 4

How many grams of oxygen are in 45 g of C₂H₂O₂? A)8.3 B)9.3 C)17 D)25 E)31

Accepted Answer

The molar mass of C₂H₂O₂ is 62 g/mol. So, 45 g of C₂H₂O₂ is equal to 45 g / 62 g/mol = 0.726 mol. Each mole of C₂H₂O₂ contains 2 moles of oxygen. So, 0.726 mol of C₂H₂O₂ contains 0.726 mol * 2 = 1.452 mol of oxygen. The molar mass of oxygen is 16 g/mol. So, 1.452 mol of oxygen is equal to 1.452 mol * 16 g/mol = 23.23 g.

Question 5

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg₃N₂ + 3 H₂O → 2NH₃ + 3MgO The yield of MgO is 3.60 g. What is the percent yield in the reaction? A)94.5 B)78.4 C)46.6 D)49.4 E)99.9

Accepted Answer

The theoretical yield of MgO can be calculated using stoichiometry. The balanced equation shows that 3 moles of MgO are produced for every 1 mole of Mg3N2. First, convert the mass of Mg3N2 to moles:
3.82 g Mg3N2 x (1 mol Mg3N2/100.95 g Mg3N2) = 0.0378 mol Mg3N2
Next, determine the limiting reactant. To do this, you need to find how many moles of MgO can be produced from 7.73 g of water. You can use the molar mass of water to convert grams to moles:
7.73 g H2O x (1 mol H2O/18.02 g H2O) x (3 mol MgO/3 mol H2O) = 0.643 mol MgO
The stoichiometry tells us that the amount of MgO produced will be limited by the amount of Mg3N2, since there is less of it than the amount of water. Therefore, 0.0378 mol Mg3N2 will produce:
0.0378 mol Mg3N2 x (3 mol MgO/1 mol Mg3N2) x (40.3 g MgO/1 mol MgO) = 4.56 g MgO (theoretical yield)
The percent yield is calculated as:
(actual yield/theoretical yield) x 100%
Plugging in the given values, we get:
(3.60 g MgO/4.56 g MgO) x 100% = 78.9%
Rounded to one decimal place, this is 78.4%. The answer is B.

Question 6

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s)+ 3 F₃ (g)→ SF₆ (g) The maximum amount of SF₆ that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is __________ g. A)12 B)3.2 C)5.8 D)16 E)8.0

Accepted Answer

To determine the maximum amount of sulfur hexafluoride that can be produced, we need to first determine which reactant is limiting. 
- Calculate the number of moles of sulfur: 
3.5 g / 32.06 g/mol = 0.109 mol 
- Calculate the number of moles of fluorine: 
4.5 g / 38.00 g/mol = 0.118 mol 
Since there are 3 moles of fluorine required for every 1 mole of sulfur, we can see that sulfur is the limiting reactant since there are fewer moles of sulfur than fluorine. 
Next, we need to determine the theoretical yield of sulfur hexafluoride: 
- Calculate the number of moles of sulfur hexafluoride that can be produced from the 0.109 moles of sulfur: 
0.109 mol sulfur × (1 mol sulfur hexafluoride / 1 mol sulfur) × (1 mol fluorine / 3 mol sulfur hexafluoride) = 0.0363 mol sulfur hexafluoride 
- Calculate the mass of sulfur hexafluoride that can be produced from the 0.0363 moles of sulfur hexafluoride: 
0.0363 mol sulfur hexafluoride × 146.06 g/mol = 5.29 g sulfur hexafluoride 
Therefore, the maximum amount of sulfur hexafluoride that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is 5.29 g. The closest answer choice is C) 5.8 g.

Question 7

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO₃ (aq)+ AlCl₃ (aq)→ Al(NO₃)₃ (aq)+ 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO₃ react with 7.73 g of AlCl₃? A)17.6 B)4.22 C)24.9 D)3.56 E)11.9

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Question 8

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s)+ 3 O₂ (g)→ 2 Al₂O₃ (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃. The % yield of the reaction is __________. A)74 B)37 C)47 D)66 E)26

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Question 9

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s)+ 3F₂ (g)→ SF₆ (g) In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a 7.90-g sample of fluorine yields __________ g of SF₆. A)30.3 B)10.1 C)7.99 D)24.0 E)0.110

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Question 10

Determine the mass percent (to the hundredths place)of Na in sodium bicarbonate (NaHCO₃).

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Question 11

If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s)+ 2 H₂O (l)→ Mg(OH)₂ (s)+ H₂ (g) A)0.0962 B)0.0162 C)0.0485 D)0.219 E)0.204

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Question 12

What is the maximum amount in grams of SO₃ that can be produced by the reaction of 1.0 g of S with 1.0 g of O₂ via the equation below? S (s)+ O₂ (g)→ SO₃ (g)(not balanced) A)0.27 B)1.7 C)2.5 D)3.8 E)2.0

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Question 13

Pentacarbonyliron (Fe(CO)₅)reacts with phosphorous trifluoride (PF₃)and hydrogen, releasing carbon monoxide: Fe(CO)₅ + PF₃ + H₂ → Fe(CO)₂(PF₃)₂(H)₂ + CO (not balanced) The reaction of 5.0 mol of Fe(CO)₅, 8.0 mol of PF₃and 6.0 mol of H₂ will release __________ mol of CO. A)15 B)5.0 C)24 D)6.0 E)12

Accepted Answer

From the balanced chemical equation, we see that for every Fe(CO)₅ molecule, one mole of CO is released. Therefore, the total moles of CO released will be equal to the initial moles of Fe(CO)₅ used. Therefore, the answer is 5.0 moles of CO.

Question 14

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g)+ 7 O₂ (g)→ 4 NO₂ (g)+ 6 H₂O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces __________ g of NO₂. A)212 B)178 C)119 D)0.954 E)43.9

Accepted Answer

1) First, we need to determine the limiting reactant:
- Convert the mass of ammonia to moles by dividing by its molar mass:
43.9 g NH3 / (17.031 g/mol NH3) = 2.578 mol NH3
- Convert the mass of oxygen to moles by dividing by its molar mass:
258 g O2 / (31.999 g/mol O2) = 8.062 mol O2
- Divide the number of moles of each reactant by their stoichiometric coefficients in the balanced equation to determine which one completely reacts:
NH3: 2.578 mol / 4 = 0.6445 mol
O2: 8.062 mol / 7 = 1.1517 mol
- The limiting reactant is ammonia because it produces less N2O per mole (0.6445 moles) compared to oxygen (1.1517 moles).

2) Determine the amount of N2O produced:
- Use the mole ratio between NH3 and N2O from the balanced equation:
4 mol N2O / 4 mol NH3 = 1 mol N2O / 1 mol NH3
- Multiply the moles of NH3 by the mole ratio to get moles of N2O produced:
0.6445 mol NH3 x 1 mol N2O / 4 mol NH3 = 0.1611 mol N2O
- Convert moles to grams by multiplying by the molar mass of N2O:
0.1611 mol N2O x 44.013 g/mol N2O = 7.087 g N2O, which rounds to 7.09 g
- The answer is closest to C) 119 g, so that must be the correct choice.

Question 15

There are __________ mol of carbon atoms in 3 mol of dimethylsulfoxide (C₂H₆SO). A)2 B)4 C)6 D)8 E)10

Accepted Answer

In dimethylsulfoxide (DMSO), the chemical formula is given as C2H6SO. It contains 2 carbon atoms. Hence, in 1 mol of DMSO, there are 2 mol of carbon atoms. Therefore, in 3 mol of DMSO, there are 6 mol of carbon atoms. Therefore, the answer is (C) 6.

Question 16

The molecular weight of acetic acid ( HC₂H₃O₂), the acid in vinegar, is __________ amu (rounded to one decimal place). A)59.0 B)29.0 C)60.1 D)8.0 E)32.0

Accepted Answer

To calculate the molecular weight of acetic acid, we need to add up the atomic weights of all the atoms in the molecule.

H: 1.01 x 4 = 4.04 
C: 12.01 x 2 = 24.02 
O: 16.00 x 2 = 32.00

Total molecular weight = 4.04 + 24.02 + 32.00 = 60.1 amu (rounded to one decimal place).

Therefore, the best choice is C.

Question 17

How many grams of hydrogen are in 23 g of CH₄O? A)2.9 B)4.6 C)2.3 D)4.0 E)5.8

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Question 18

Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃ (s)→ PbO (s)+ CO₂ (g) If the reaction yield is 95.7%, how many grams of lead (II)oxide will be produced by the decomposition of 2.50 g of lead (II)carbonate? A)1.04 B)1.55 C)2.09 D)4.00 E)5.55

Accepted Answer

First, we need to calculate the theoretical yield of lead (II)oxide:

1 mole of PbCO3 produces 1 mole of PbO

Molar mass of PbCO3 = 267.2 g/mol
1 mole of PbCO3 = 267.2 g

Therefore, 2.50 g of PbCO3 is equal to:

2.50 g PbCO3 x (1 mol PbCO3 / 267.2 g PbCO3) = 0.00936 mol PbCO3

Since the reaction yield is 95.7%, the actual yield of PbO is:

0.0957 x theoretical yield

0.0957 x 0.00936 mol PbO = 0.000895 mol PbO

Finally, we need to convert moles of PbO to grams:

Molar mass of PbO = 223.2 g/mol
0.000895 mol PbO x 223.2 g/mol = 0.1995 g PbO

Therefore, the answer is:

C) 2.09

Question 19

How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water? Mg₃N₂ + 3 H₂O → 2NH₃ + 3MgO A)0.114 B)0.0378 C)0.429 D)0.0756 E)4.57

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Question 20

What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N₂ with 3.0 g of H₂ via the equation below? N₂ (g)+ H₂ (g)→ NH₃ (g)(not balanced) A)2.0 B)1.2 C)0.61 D)17 E)4.0

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Quiz 3: Stoichiometry: Calculations With Chemical Formulas and Equations

What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2 H₂O (l) → Mg(OH) ₂ (s) + H₂ (g)

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s) + 3O₂ (g) → 2SO₃ (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O₂ produced 0.80 g of SO₃. The % yield in this experiment is __________.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3 O₂ (g) → 2 Al₂O₃ (s) The maximum amount of Al₂O₃ that can be produced from 2.5 g of Al and 2.5 g of O₂ is __________ g.

How many grams of oxygen are in 45 g of C₂H₂O₂?

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg₃N₂ + 3 H₂O → 2NH₃ + 3MgO The yield of MgO is 3.60 g. What is the percent yield in the reaction?

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3 F₃ (g) → SF₆ (g) The maximum amount of SF₆ that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is __________ g.

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO₃ (aq) + AlCl₃ (aq) → Al(NO₃) ₃ (aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO₃ react with 7.73 g of AlCl₃?

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3 O₂ (g) → 2 Al₂O₃ (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃. The % yield of the reaction is __________.

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F₂ (g) → SF₆ (g) In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a 7.90-g sample of fluorine yields __________ g of SF₆.

Determine the mass percent (to the hundredths place)of Na in sodium bicarbonate (NaHCO₃).

If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2 H₂O (l) → Mg(OH) ₂ (s) + H₂ (g)

What is the maximum amount in grams of SO₃ that can be produced by the reaction of 1.0 g of S with 1.0 g of O₂ via the equation below? S (s) + O₂ (g) → SO₃ (g) (not balanced)

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g) + 7 O₂ (g) → 4 NO₂ (g) + 6 H₂O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces __________ g of NO₂.

There are __________ mol of carbon atoms in 3 mol of dimethylsulfoxide (C₂H₆SO) .

The molecular weight of acetic acid ( HC₂H₃O₂) , the acid in vinegar, is __________ amu (rounded to one decimal place) .

How many grams of hydrogen are in 23 g of CH₄O?

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂ (g) If the reaction yield is 95.7%, how many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water? Mg₃N₂ + 3 H₂O → 2NH₃ + 3MgO

What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N₂ with 3.0 g of H₂ via the equation below? N₂ (g) + H₂ (g) → NH₃ (g) (not balanced)

Quiz 3: Stoichiometry: Calculations With Chemical Formulas and Equations

What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2 H2O (l) → Mg(OH) 2 (s) + H2 (g)

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s) + 3O2 (g) → 2SO3 (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is __________.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3 O2 (g) → 2 Al2O3 (s) The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is __________ g.

How many grams of oxygen are in 45 g of C2H2O2?

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg3N2 + 3 H2O → 2NH3 + 3MgO The yield of MgO is 3.60 g. What is the percent yield in the reaction?

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3 F3 (g) → SF6 (g) The maximum amount of SF6 that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is __________ g.

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO3 (aq) + AlCl3 (aq) → Al(NO3) 3 (aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3?

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3 O2 (g) → 2 Al2O3 (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The % yield of the reaction is __________.

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F2 (g) → SF6 (g) In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a 7.90-g sample of fluorine yields __________ g of SF6.

Determine the mass percent (to the hundredths place)of Na in sodium bicarbonate (NaHCO3).

If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2 H2O (l) → Mg(OH) 2 (s) + H2 (g)

What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0 g of S with 1.0 g of O2 via the equation below? S (s) + O2 (g) → SO3 (g) (not balanced)

Pentacarbonyliron (Fe(CO) 5) reacts with phosphorous trifluoride (PF3) and hydrogen, releasing carbon monoxide: Fe(CO) 5 + PF3 + H2 → Fe(CO) 2(PF3) 2(H) 2 + CO (not balanced) The reaction of 5.0 mol of Fe(CO) 5, 8.0 mol of PF3and 6.0 mol of H2 will release __________ mol of CO.

The combustion of ammonia in the presence of oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces __________ g of NO2.

There are __________ mol of carbon atoms in 3 mol of dimethylsulfoxide (C2H6SO) .

The molecular weight of acetic acid ( HC2H3O2) , the acid in vinegar, is __________ amu (rounded to one decimal place) .

How many grams of hydrogen are in 23 g of CH4O?

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) If the reaction yield is 95.7%, how many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water? Mg3N2 + 3 H2O → 2NH3 + 3MgO

What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N2 with 3.0 g of H2 via the equation below? N2 (g) + H2 (g) → NH3 (g) (not balanced)

What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2 H₂O (l) → Mg(OH) ₂ (s) + H₂ (g)

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s) + 3O₂ (g) → 2SO₃ (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O₂ produced 0.80 g of SO₃. The % yield in this experiment is __________.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3 O₂ (g) → 2 Al₂O₃ (s) The maximum amount of Al₂O₃ that can be produced from 2.5 g of Al and 2.5 g of O₂ is __________ g.

How many grams of oxygen are in 45 g of C₂H₂O₂?

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg₃N₂ + 3 H₂O → 2NH₃ + 3MgO The yield of MgO is 3.60 g. What is the percent yield in the reaction?

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3 F₃ (g) → SF₆ (g) The maximum amount of SF₆ that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is __________ g.

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO₃ (aq) + AlCl₃ (aq) → Al(NO₃) ₃ (aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO₃ react with 7.73 g of AlCl₃?

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3 O₂ (g) → 2 Al₂O₃ (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃. The % yield of the reaction is __________.

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F₂ (g) → SF₆ (g) In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a 7.90-g sample of fluorine yields __________ g of SF₆.

Determine the mass percent (to the hundredths place)of Na in sodium bicarbonate (NaHCO₃).

If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2 H₂O (l) → Mg(OH) ₂ (s) + H₂ (g)

What is the maximum amount in grams of SO₃ that can be produced by the reaction of 1.0 g of S with 1.0 g of O₂ via the equation below? S (s) + O₂ (g) → SO₃ (g) (not balanced)

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g) + 7 O₂ (g) → 4 NO₂ (g) + 6 H₂O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces __________ g of NO₂.

There are __________ mol of carbon atoms in 3 mol of dimethylsulfoxide (C₂H₆SO) .

The molecular weight of acetic acid ( HC₂H₃O₂) , the acid in vinegar, is __________ amu (rounded to one decimal place) .

How many grams of hydrogen are in 23 g of CH₄O?

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂ (g) If the reaction yield is 95.7%, how many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water? Mg₃N₂ + 3 H₂O → 2NH₃ + 3MgO

What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N₂ with 3.0 g of H₂ via the equation below? N₂ (g) + H₂ (g) → NH₃ (g) (not balanced)