Question 1

Sulfur and oxygen react to produce sulfur trioxide.In a particular experiment,7.9 grams of SO₃are produced by the reaction of 6.0 grams of O₂ with 7.0 grams of S.What is the % yield of SO₃ in this experiment? S (s)+ O₂(g)→ SO₃ (g)(not balanced)

Accepted Answer

First, we need to balance the equation to determine the mole ratio between S and SO2:
2S (s) + 3O2 (g) → 2SO3 (g)

Next, we need to calculate the theoretical yield of SO3 using the mole ratio and the limiting reactant (S):
Moles of S used = 7.0 g / 32.06 g/mol = 0.218 mol
Moles of SO3 produced = 2 * 0.218 mol = 0.436 mol
Theoretical yield of SO3 = 0.436 mol * 80.06 g/mol = 34.92 g

Finally, we can calculate the percent yield:
% Yield = (Actual yield / Theoretical yield) x 100%
Actual yield = 7.9 g
% Yield = (7.9 g / 34.92 g) x 100% = 22.6%

The closest answer choice to this calculation is D) 79.

Question 2

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂(s)+ 2H₂O (g)→ Ca(OH)₂ (s)+ C₂H₂ (g) Production of 6.5 g of C₂H₂ requires consumption of ________ g of H₂O.

Accepted Answer

To solve this, first, we need to balance the chemical equation and then use stoichiometry to find the mass of water consumed. The balanced chemical equation is already given: $$CaC_2(s) + 2H_2O(g) \rightarrow Ca(OH)_2(s) + C_2H_2(g)$$. This shows a 1:2 molar ratio between calcium carbide and water. The molar mass of acetylene ($C_2H_2$) is approximately 26 g/mol. Therefore, to produce 6.5 g of acetylene, $\frac{6.5 \, \text{g}}{26 \, \text{g/mol}} = 0.25 \, \text{mol}$ of acetylene are produced. Since the reaction requires 2 moles of water for every mole of acetylene produced, we need $0.25 \, \text{mol} \times 2 = 0.5 \, \text{mol}$ of water. The molar mass of water ($H_2O$) is approximately 18 g/mol, so $0.5 \, \text{mol} \times 18 \, \text{g/mol} = 9.0 \, \text{g}$ of water are consumed.

Question 3

The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide.The combustion of 10 mol of CS₂ in the presence of excess oxygen yields ________ mol of SO₂.

Accepted Answer

The answer of The combustion of carbon disulfide in the...

Question 4

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.A 18.2 g sample of hydrogen requires ________ g of N₂for a complete reaction.

Accepted Answer

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Question 5

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s)+ H₂O (l)→ Ca(OH)₂(s) A 3.50 g sample of CaO is reacted with 3.38 g of H₂O.How many grams of water remain after completion of reaction?

Accepted Answer

First, we need to determine the limiting reactant in the reaction. To do this, we can use stoichiometry and convert both reactants to moles of calcium hydroxide produced:

For CaO:
3.50 g CaO x (1 mol CaO/56.08 g CaO) x (1 mol Ca(OH)2/1 mol CaO) = 0.0625 mol Ca(OH)2

For H2O:
3.38 g H2O x (1 mol H2O/18.02 g H2O) x (1 mol Ca(OH)2/1 mol H2O) = 0.1875 mol Ca(OH)2

Since CaO produces the smaller amount of Ca(OH)2, it is the limiting reactant. This means that all of the CaO will react and be converted to Ca(OH)2, while some of the water will remain unreacted.

To determine the amount of water remaining, we can use stoichiometry again and calculate how much water is required to react with 0.0625 mol of CaO (the amount originally present):

0.0625 mol CaO x (1 mol H2O/1 mol CaO) x (18.02 g H2O/1 mol H2O) = 1.125 g H2O

Since we started with 3.38 g of water and only 1.125 g was required for the reaction, the remaining amount is:

3.38 g - 1.125 g = 2.255 g

Therefore, the answer is choice C: 2.25 g.

Question 6

Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃(s)→ PbO (s)+ CO₂(g) ________ grams of lead (II)oxide will be produced by the decomposition of 8.75 g of lead (II)carbonate?

Accepted Answer

To solve this problem, we first need to balance the chemical equation and then use stoichiometry to find the mass of lead (II) oxide produced. The balanced equation for the decomposition of lead (II) carbonate (PbCO3) into lead (II) oxide (PbO) and carbon dioxide (CO2) is:$$ \text{PbCO}_3 (s) \rightarrow \text{PbO} (s) + \text{CO}_2 (g) $$Next, we calculate the molar mass of lead (II) carbonate and lead (II) oxide:- Molar mass of PbCO3 = 207.2 (Pb) + 12.01 (C) + 3*16.00 (O) = 267.21 g/mol- Molar mass of PbO = 207.2 (Pb) + 16.00 (O) = 223.2 g/molGiven 8.75 g of PbCO3, we find the moles of PbCO3:$$ \text{Moles of PbCO}_3 = \frac{8.75 \text{ g}}{267.21 \text{ g/mol}} = 0.0327 \text{ mol} $$Since the reaction is a 1:1 mole ratio between PbCO3 and PbO, the moles of PbO produced will also be 0.0327 mol. To find the mass of PbO produced:$$ \text{Mass of PbO} = 0.0327 \text{ mol} \times 223.2 \text{ g/mol} = 7.30 \text{ g} $$Therefore, 7.31 grams of lead (II) oxide will be produced by the decomposition of 8.75 g of lead (II) carbonate.

Question 7

The empirical weight is always a whole-number multiple of the molecular formula weight.

Accepted Answer

The empirical formula weight is always a whole-number multiple of the molecular formula weight, not the other way around. The empirical formula represents the simplest whole-number ratio of atoms in a compound, while the molecular formula represents the actual number of atoms of each element in a molecule of the compound.

Question 8

If 588 grams of FeS₂ is allowed to react with 352 grams of O₂according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂+ O₂ → Fe₂O₃ + SO₂

Accepted Answer

The answer of If 588 grams of FeS₂ is allowed...

Question 9

The mass of a single atom of an element (in amu)is numerically equal to the mass in grams of that element.

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Question 10

Water can be formed from the stoichiometric reaction of hydrogen with oxygen.How many grams of H₂O is generated when 45.3 g of O₂reacts with excess hydrogen?

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Question 11

Complete and balance the following reaction,given that elemental sodium reacts with elemental oxygen to form Na₂O (s). K (s)+ S (s)→ ________

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Question 12

The quantity of product that is calculated to form when all of the limiting reagent reacts is called the percent yield.

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Question 13

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s)+ O₂(g)→ 2MgO (s) When 5.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Accepted Answer

The answer of Magnesium burns in air with a dazzling...

Question 14

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s)+ H₂O (l)→ Ca(OH)₂(s) In a particular experiment,a 2.00-g sample of CaO is reacted with excess water and 2.14 g of Ca(OH)₂ is recovered.What is the percent yield in this experiment?

Accepted Answer

The answer of Calcium oxide reacts with water in a...

Question 15

The combustion of propane (C₃H₈)in the presence of excess oxygen yields CO₂ and H₂O: C₃H₈ (g)+ 5O₂ (g)→ 3CO₂(g)+ 4H₂O (g) How many grams of CO₂ is produced when 12.5 g of C₃H₈ burns in open air?

Accepted Answer

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Question 16

A compound was found to contain 90.6% lead (Pb)and 9.4% oxygen.The empirical formula for this compound is ________.

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The answer of A compound was found to contain 90.6%...

Question 17

A great deal of oxygen is produced during combustion.

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Question 18

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s)+ N₂(g)→ 2Li₃N (s) In a particular experiment,2.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Accepted Answer

The answer of Lithium and nitrogen react in a combination...

Quiz 3: Chemical Reactions and Reaction Stoichiometry

Sulfur and oxygen react to produce sulfur trioxide.In a particular experiment,7.9 grams of SO₃are produced by the reaction of 6.0 grams of O₂ with 7.0 grams of S.What is the % yield of SO₃ in this experiment? S (s) + O₂(g) → SO₃ (g) (not balanced)

Calcium carbide (CaC₂) reacts with water to produce acetylene (C₂H₂) : CaC₂(s) + 2H₂O (g) → Ca(OH) ₂ (s) + C₂H₂ (g) Production of 6.5 g of C₂H₂ requires consumption of ________ g of H₂O.

The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide.The combustion of 10 mol of CS₂ in the presence of excess oxygen yields ________ mol of SO₂.

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.A 18.2 g sample of hydrogen requires ________ g of N₂for a complete reaction.

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H₂O (l) → Ca(OH) ₂(s) A 3.50 g sample of CaO is reacted with 3.38 g of H₂O.How many grams of water remain after completion of reaction?

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃(s) → PbO (s) + CO₂(g) ________ grams of lead (II) oxide will be produced by the decomposition of 8.75 g of lead (II) carbonate?

The empirical weight is always a whole-number multiple of the molecular formula weight.

If 588 grams of FeS₂ is allowed to react with 352 grams of O₂according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂+ O₂ → Fe₂O₃ + SO₂

The mass of a single atom of an element (in amu)is numerically equal to the mass in grams of that element.

Water can be formed from the stoichiometric reaction of hydrogen with oxygen.How many grams of H₂O is generated when 45.3 g of O₂reacts with excess hydrogen?

Complete and balance the following reaction,given that elemental sodium reacts with elemental oxygen to form Na₂O (s). K (s)+ S (s)→ ________

The quantity of product that is calculated to form when all of the limiting reagent reacts is called the percent yield.

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O₂(g) → 2MgO (s) When 5.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H₂O (l) → Ca(OH) ₂(s) In a particular experiment,a 2.00-g sample of CaO is reacted with excess water and 2.14 g of Ca(OH) ₂ is recovered.What is the percent yield in this experiment?

The combustion of propane (C₃H₈)in the presence of excess oxygen yields CO₂ and H₂O: C₃H₈ (g)+ 5O₂ (g)→ 3CO₂(g)+ 4H₂O (g) How many grams of CO₂ is produced when 12.5 g of C₃H₈ burns in open air?

A compound was found to contain 90.6% lead (Pb)and 9.4% oxygen.The empirical formula for this compound is ________.

A great deal of oxygen is produced during combustion.

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N₂(g) → 2Li₃N (s) In a particular experiment,2.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Quiz 3: Chemical Reactions and Reaction Stoichiometry

Sulfur and oxygen react to produce sulfur trioxide.In a particular experiment,7.9 grams of SO3 are produced by the reaction of 6.0 grams of O2 with 7.0 grams of S.What is the % yield of SO3 in this experiment? S (s) + O2 (g) → SO3 (g) (not balanced)

Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2) : CaC2 (s) + 2H2O (g) → Ca(OH) 2 (s) + C2H2 (g) Production of 6.5 g of C2H2 requires consumption of ________ g of H2O.

The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide.The combustion of 10 mol of CS2 in the presence of excess oxygen yields ________ mol of SO2.

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.A 18.2 g sample of hydrogen requires ________ g of N2 for a complete reaction.

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H2O (l) → Ca(OH) 2 (s) A 3.50 g sample of CaO is reacted with 3.38 g of H2O.How many grams of water remain after completion of reaction?

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) ________ grams of lead (II) oxide will be produced by the decomposition of 8.75 g of lead (II) carbonate?

The empirical weight is always a whole-number multiple of the molecular formula weight.

If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the following unbalanced equation,how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

The mass of a single atom of an element (in amu)is numerically equal to the mass in grams of that element.

Water can be formed from the stoichiometric reaction of hydrogen with oxygen.How many grams of H2O is generated when 45.3 g of O2 reacts with excess hydrogen?

Complete and balance the following reaction,given that elemental sodium reacts with elemental oxygen to form Na2O (s). K (s)+ S (s)→ ________

The quantity of product that is calculated to form when all of the limiting reagent reacts is called the percent yield.

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2 (g) → 2MgO (s) When 5.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H2O (l) → Ca(OH) 2 (s) In a particular experiment,a 2.00-g sample of CaO is reacted with excess water and 2.14 g of Ca(OH) 2 is recovered.What is the percent yield in this experiment?

The combustion of propane (C3H8)in the presence of excess oxygen yields CO2 and H2O: C3H8 (g)+ 5O2 (g)→ 3CO2 (g)+ 4H2O (g) How many grams of CO2 is produced when 12.5 g of C3H8 burns in open air?

A compound was found to contain 90.6% lead (Pb)and 9.4% oxygen.The empirical formula for this compound is ________.

A great deal of oxygen is produced during combustion.

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N2 (g) → 2Li3N (s) In a particular experiment,2.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Sulfur and oxygen react to produce sulfur trioxide.In a particular experiment,7.9 grams of SO₃are produced by the reaction of 6.0 grams of O₂ with 7.0 grams of S.What is the % yield of SO₃ in this experiment? S (s) + O₂(g) → SO₃ (g) (not balanced)

Calcium carbide (CaC₂) reacts with water to produce acetylene (C₂H₂) : CaC₂(s) + 2H₂O (g) → Ca(OH) ₂ (s) + C₂H₂ (g) Production of 6.5 g of C₂H₂ requires consumption of ________ g of H₂O.

The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide.The combustion of 10 mol of CS₂ in the presence of excess oxygen yields ________ mol of SO₂.

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.A 18.2 g sample of hydrogen requires ________ g of N₂for a complete reaction.

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H₂O (l) → Ca(OH) ₂(s) A 3.50 g sample of CaO is reacted with 3.38 g of H₂O.How many grams of water remain after completion of reaction?

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃(s) → PbO (s) + CO₂(g) ________ grams of lead (II) oxide will be produced by the decomposition of 8.75 g of lead (II) carbonate?

If 588 grams of FeS₂ is allowed to react with 352 grams of O₂according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂+ O₂ → Fe₂O₃ + SO₂

Water can be formed from the stoichiometric reaction of hydrogen with oxygen.How many grams of H₂O is generated when 45.3 g of O₂reacts with excess hydrogen?

Complete and balance the following reaction,given that elemental sodium reacts with elemental oxygen to form Na₂O (s). K (s)+ S (s)→ ________

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O₂(g) → 2MgO (s) When 5.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H₂O (l) → Ca(OH) ₂(s) In a particular experiment,a 2.00-g sample of CaO is reacted with excess water and 2.14 g of Ca(OH) ₂ is recovered.What is the percent yield in this experiment?

The combustion of propane (C₃H₈)in the presence of excess oxygen yields CO₂ and H₂O: C₃H₈ (g)+ 5O₂ (g)→ 3CO₂(g)+ 4H₂O (g) How many grams of CO₂ is produced when 12.5 g of C₃H₈ burns in open air?

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N₂(g) → 2Li₃N (s) In a particular experiment,2.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.