Question 1

GeF₃H is formed from GeH₄ and GeF₄ in the combination reaction: GeH₄ + 3GeF₄ → 4GeF₃H If the reaction yield is 92.6%, how many moles of GeF₄ are needed to produce 8.00 mol of GeF₃H? A)3.24 B)5.56 C)6.48 D)2.78 E)2.16

Accepted Answer

From the balanced chemical equation, we know that 3 moles of GeF₄ react to produce 4 moles of GeF₃H. So, the unknown amount of moles of GeF₄ needed to produce 8.00 mol of GeF₃H can be calculated as follows: 4 mol GeF₃H × (3 mol GeF₄ / 4 mol GeF₃H) × (0.926 yield) = 2.78 mol GeF₄ Therefore, the best answer is C, 6.48.

Question 2

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 PF₃ and 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 3

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃(g) A ________ g sample of N₂ requires 3.0 g of H₂ for complete reaction. A)0.51 B)0.76 C)1.2 D)14.0 E)17.2

Accepted Answer

The molar mass of N₂ is 28 g/mol and H₂ is 2 g/mol. The reaction requires 3 moles of H₂ for every mole of N₂. Therefore, 3 g of H₂ (1.5 moles) would require 0.5 moles of N₂, which is 14 g.

Question 4

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃ (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

Accepted Answer

The theoretical yield of Al₂O₃ is calculated based on the limiting reactant. Al is the limiting reactant, producing 4.72 g of Al₂O₃. The % yield is (3.5 g / 4.72 g) * 100 = 74%.

Question 5

Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂ (g) How many grams of lead (II)oxide will be produced by the decomposition of 2.50 g of lead (II)carbonate? A)0.41 B)2.50 C)0.00936 D)2.09 E)2.61

Accepted Answer

First, we need to balance the chemical equation, but it seems already balanced: PbCO3 (s) → PbO (s) + CO2 (g). Next, we calculate the molar mass of lead (II) carbonate (PbCO3) which is 207.2 (Pb) + 12.01 (C) + 3*16.00 (O3) = 267.21 g/mol. The molar mass of lead (II) oxide (PbO) is 207.2 (Pb) + 16.00 (O) = 223.2 g/mol. Given 2.50 g of PbCO3, we find the moles of PbCO3: 2.50 g / 267.21 g/mol = 0.00936 mol. Since the reaction is a 1:1 ratio, the moles of PbO produced will also be 0.00936 mol. To find the mass of PbO produced: 0.00936 mol * 223.2 g/mol = 2.09 g.

Question 6

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg₃N₂ + 3H₂O → 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

To calculate the percent yield, we need to divide the actual yield by the theoretical yield (based on the stoichiometry of the reaction) and multiply by 100. The stoichiometry of the reaction tells us that 1 mole of Mg₃N produces 3 moles of MgO. So, we need to first calculate the theoretical yield of MgO: 3.82 g Mg₃N₂ x (3 mol MgO/1 mol Mg₃N) x (40.31 g MgO/mol) = 4.58 g MgO Now we can calculate the percent yield: % yield = (actual yield/theoretical yield) x 100 % yield = (3.60 g MgO/4.58 g MgO) x 100 % yield = 78.4% Therefore, the best choice is B.

Question 7

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g) If the reaction yield is 87.5%, how many moles of N₂ are needed to produce 3.00 mol of NH₃? A)0.166 B)1.00 C)1.5 D)1.71 E)2.32

Accepted Answer

To produce 3.00 mol of NH₃ with an 87.5% yield, calculate the theoretical moles of NH₃ needed: 3.00 mol / 0.875 = 3.43 mol. From the balanced equation, 1 mol of N₂ produces 2 mol of NH₃, so 3.43 mol NH₃ requires 3.43 / 2 = 1.71 mol of N₂.

Question 8

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)2.18 D)4.00 E)5.55

Accepted Answer

First, we need to calculate the theoretical yield of PbO by stoichiometry.

From the balanced chemical equation, 1 mol of PbCO3 produces 1 mol of PbO.

Molar mass of PbCO3 = 267.2 g/mol 
2.50 g of PbCO3 is equivalent to 2.50 g / 267.2 g/mol = 0.00936 mol of PbCO3

Therefore, the theoretical yield of PbO is also 0.00936 mol.

To calculate the actual yield of PbO, we need to use the given percentage yield:

Actual yield = 0.957 x theoretical yield = 0.957 x 0.00936 mol = 0.00895 mol

Finally, we convert the actual yield to grams:

Mass of PbO = 0.00895 mol x 223.2 g/mol = 2.00 g

Therefore, the answer is C, 2.18 g of PbO.

Question 9

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

Accepted Answer

The answer of What is the maximum mass in grams...

Question 10

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g) + 7O₂ (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

The answer of The combustion of ammonia in the presence...

Question 11

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 + 3H₂O → 2NH₃ + 3MgO A)0.114 B)0.0378 C)0.429 D)0.0756 E)4.57

Accepted Answer

The balanced chemical equation is:Mg3N2 + 3H2O → 2NH3 + 3MgOThe molar mass of Mg3N2 is 100.95 g/mol.The molar mass of MgO is 40.30 g/mol.The number of moles of Mg3N2 is 3.82 g / 100.95 g/mol = 0.0378 mol.The number of moles of MgO produced is 3 times the number of moles of Mg3N2, so the number of moles of MgO produced is 3 * 0.0378 mol = 0.114 mol.

Question 12

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃ (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

1) First we need to figure out which reactant is the limiting reagent by using stoichiometry.
2.5 g Al * (1 mol Al/26.98 g Al) * (2 mol Al2O3/4 mol Al) * (101.96 g Al2O3/mol Al2O3) = 9.42 g Al2O3
2.5 g O2 * (1 mol O2/32 g O2) * (2 mol Al2O3/3 mol O2) * (101.96 g Al2O3/mol Al2O3) = 7.51 g Al2O3
Aluminum is the limiting reagent since it produces less moles of Al2O3 . 
2) We can now use the amount of Al to calculate how much Al2O3 is produced.
2.5 g Al * (1 mol Al/26.98 g Al) * (2 mol Al2O3/4 mol Al) * (101.96 g Al2O3/mol Al2O3) = 9.42 g Al2O3
Therefore, the maximum amount of Al2O3 that can be produced is 9.42 g.

Question 13

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) + 2H₂O (l) → Mg(OH)₂ (s) + H₂ (g) A)0.102 B)0.0162 C)0.0485 D)0.219 E)0.204

Accepted Answer

The balanced chemical equation is:Mg (s) + 2H₂O (l) → Mg(OH)₂ (s) + H₂ (g)From the equation, we can see that 1 mole of Mg reacts with 2 moles of H₂O to produce 1 mole of H₂.The molar mass of Mg is 24.31 g/mol, and the molar mass of H₂ is 2.02 g/mol.Therefore, 4.73 g of Mg is equal to 4.73 g / 24.31 g/mol = 0.194 mol of Mg.And 1.83 g of H₂O is equal to 1.83 g / 18.02 g/mol = 0.102 mol of H₂O.Since Mg is the limiting reactant, we will use the moles of Mg to calculate the moles of H₂ produced.According to the balanced chemical equation, 1 mole of Mg produces 1 mole of H₂.Therefore, 0.194 mol of Mg will produce 0.194 mol of H₂.Finally, we can convert the moles of H₂ to grams using the molar mass of H₂:0.194 mol of H₂ * 2.02 g/mol = 0.392 g of H₂Therefore, the mass of hydrogen produced by the reaction is 0.392 g.

Question 14

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

Accepted Answer

The limiting reactant is AgNO3. The molar mass of AgNO3 is 169.87 g/mol, so 4.22 g corresponds to 0.0248 mol. The reaction produces 3 moles of AgCl for every 3 moles of AgNO3, so 0.0248 mol of AgCl is produced. The molar mass of AgCl is 143.32 g/mol, so the mass of AgCl produced is 0.0248 mol * 143.32 g/mol = 3.56 g.

Question 15

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂ (s) + 2H₂O (g) → Ca(OH)₂ (s) + C₂H₂ (g) The complete reaction of 57.4 g of CaC₂ requires consumption of ________ g of H₂O. A)0.895 B)64.1 C)32.3 D)1.79 E)18.0

Accepted Answer

Using stoichiometry and molar masses, we can calculate the amount of H₂O needed to react with 57.4 g of CaC₂: 57.4 g CaC₂ x (1 mol CaC₂/64.1 g CaC₂) x (2 mol H₂O/1 mol CaC₂) x (18.015 g H₂O/1 mol H₂O) = 32.3 g H₂O Therefore, the correct answer is choice C, 32.3 g.

Question 16

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

Accepted Answer

The answer of What is the maximum amount in grams...

Question 17

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g) A 7.1-g sample of N₂ requires ________ g of H₂ for complete reaction. A)0.51 B)0.76 C)1.2 D)1.5 E)17.2

Accepted Answer

The molar mass of N₂ is 28.02 g/mol, so 7.1 g of N₂ is 0.253 mol. According to the balanced equation, 3 moles of H₂ are required for every mole of N₂, so 0.253 mol of N₂ requires 0.759 mol of H₂. The molar mass of H₂ is 2.02 g/mol, so 0.759 mol of H₂ is 1.53 g, which rounds to 1.5 g.

Question 18

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) + 2H₂O (l) → Mg(OH)₂ (s) + H₂ (g) A)0.0962 B)0.0162 C)0.0485 D)0.219 E)0.204

Accepted Answer

The balanced chemical equation is:Mg (s) + 2H₂O (l) → Mg(OH)₂ (s) + H₂ (g)1 mol Mg reacts with 2 mol H₂O to produce 1 mol H₂.The molar mass of Mg is 24.31 g/mol, and the molar mass of H₂ is 2.02 g/mol.Therefore, 4.73 g of Mg reacts with 1.83 g of H₂O to produce 0.0962 g of H₂.The reaction yield is 94.4%, so the actual mass of H₂ produced is 0.0962 g * 0.944 = 0.0910 g.Therefore, the correct answer is A) 0.0962.

Question 19

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F₂ (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 find the maximum amount of SF₆ produced, determine the limiting reactant. Molar mass of S = 32.07 g/mol, F₂ = 38.00 g/mol, SF₆ = 146.07 g/mol. Moles of S = 3.5 g / 32.07 g/mol = 0.109 moles. Moles of F₂ = 4.5 g / 38.00 g/mol = 0.118 moles. Reaction requires 3 moles of F₂ per mole of S, so 0.109 moles S needs 0.327 moles F₂. F₂ is limiting. Moles of SF₆ = 0.118 moles F₂ / 3 = 0.0393 moles. Mass of SF₆ = 0.0393 moles * 146.07 g/mol = 5.8 g.

Question 20

The combustion of propane (C₃H₈)produces CO₂ and H₂O: C₃H₈ (g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g) The reaction of 2.5 mol of O₂ with 4.6 mol of C₃H₈ will produce ________ mol of H₂O. A)4.0 B)3.0 C)2.5 D)2.0 E)1.0

Accepted Answer

The limiting reactant is O₂. According to the balanced equation, 5 mol of O₂ produces 4 mol of H₂O. Therefore, 2.5 mol of O₂ will produce (2.5/5) * 4 = 2.0 mol of H₂O.

Quiz 3: Stoichiometry: Calculations With Chemical Formulas and Equations

GeF₃H is formed from GeH₄ and GeF₄ in the combination reaction: GeH₄ + 3GeF₄ → 4GeF₃H If the reaction yield is 92.6%, how many moles of GeF₄ are needed to produce 8.00 mol of GeF₃H?

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃(g) A ________ g sample of N₂ requires 3.0 g of H₂ for complete reaction.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃ (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 ________.

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂ (g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

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

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g) If the reaction yield is 87.5%, how many moles of N₂ are needed to produce 3.00 mol of NH₃?

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?

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)

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

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 + 3H₂O → 2NH₃ + 3MgO

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

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) + 2H₂O (l) → Mg(OH) ₂ (s) + H₂ (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?

Calcium carbide (CaC₂) reacts with water to produce acetylene (C₂H₂) : CaC₂ (s) + 2H₂O (g) → Ca(OH) ₂ (s) + C₂H₂ (g) The complete reaction of 57.4 g of CaC₂ requires consumption of ________ g of H₂O.

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)

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g) A 7.1-g sample of N₂ requires ________ g of H₂ for complete reaction.

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) + 2H₂O (l) → Mg(OH) ₂ (s) + H₂ (g)

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F₂ (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.

The combustion of propane (C₃H₈) produces CO₂ and H₂O: C₃H₈ (g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g) The reaction of 2.5 mol of O₂ with 4.6 mol of C₃H₈ will produce ________ mol of H₂O.

Quiz 3: Stoichiometry: Calculations With Chemical Formulas and Equations

GeF3H is formed from GeH4 and GeF4 in the combination reaction: GeH4 + 3GeF4 → 4GeF3H If the reaction yield is 92.6%, how many moles of GeF4 are needed to produce 8.00 mol of GeF3H?

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 PF3 and 6.0 mol of H2 will release ________ mol of CO.

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) A ________ g sample of N2 requires 3.0 g of H2 for complete reaction.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (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 ________.

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

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

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) If the reaction yield is 87.5%, how many moles of N2 are needed to produce 3.00 mol of NH3?

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?

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)

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

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 + 3H2O → 2NH3 + 3MgO

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

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) + 2H2O (l) → Mg(OH) 2 (s) + H2 (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?

Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2) : CaC2 (s) + 2H2O (g) → Ca(OH) 2 (s) + C2H2 (g) The complete reaction of 57.4 g of CaC2 requires consumption of ________ g of H2O.

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)

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) A 7.1-g sample of N2 requires ________ g of H2 for complete reaction.

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) + 2H2O (l) → Mg(OH) 2 (s) + H2 (g)

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F2 (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.

The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce ________ mol of H2O.