Question 1

Determine the theoretical yield of H₂S (in moles)if 16 mol Al₂S₃ and 16 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃= 150.17 g/mol. Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

Accepted Answer

The answer of Determine the theoretical yield of H₂S (in...

Question 2

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

Accepted Answer

The mass of water involved can be found using the law of conservation of mass. The total mass before the reaction (sodium + water) equals the total mass after the reaction (hydrogen + sodium hydroxide). Given 17.94 g of sodium reacts to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide, the mass of water can be calculated as: mass of water = (0.78 g + 31.20 g) - 17.94 g = 32.98 g - 17.94 g = 14.04 g.

Question 3

When 14.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ H₂(g)

Accepted Answer

Step 1: Calculate the theoretical yield of calcium hydroxide:

Moles of Ca = mass/Molar mass = 14.0 g/40.08 g/mol = 0.349 mol

Moles of Ca(OH)2 = 0.349 mol/1 = 0.349 mol

Mass of Ca(OH)2 = moles × molar mass = 0.349 mol × (74.09 + 2(15.999)) g/mol = 26.56 g

Step 2: Calculate the percent yield:

% yield = (actual yield/theoretical yield) × 100%

actual yield = 5.00 g

theoretical yield = 26.56 g

% yield = (5.00 g/26.56 g) × 100% = 18.8%

Therefore, the closest answer is B) 19.3% (rounded to one decimal place).

Question 4

Describe the greenhouse effect.

Accepted Answer

The answer of Describe the greenhouse effect....

Question 5

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Accepted Answer

First, we need to write the balanced chemical equation for the reaction: $ \text{2AgNO}_3 + \text{BaCl}_2 \rightarrow 2\text{AgCl} + \text{Ba(NO}_3)_2 $.Next, we calculate the molar masses of the reactants and products involved in the reaction:- Molar mass of $ \text{AgNO}_3 $ = 169.87 g/mol- Molar mass of $ \text{BaCl}_2 $ = 208.23 g/mol- Molar mass of $ \text{AgCl} $ = 143.32 g/molUsing the given masses of the reactants, we find the moles of each reactant:- Moles of $ \text{AgNO}_3 $ = $ \frac{10.2 \text{ g}}{169.87 \text{ g/mol}} $ = 0.0600 mol- Moles of $ \text{BaCl}_2 $ = $ \frac{15.0 \text{ g}}{208.23 \text{ g/mol}} $ = 0.0720 molFrom the balanced equation, we see that 2 moles of $ \text{AgNO}_3 $ react with 1 mole of $ \text{BaCl}_2 $. Therefore, $ \text{AgNO}_3 $ is the limiting reactant in this case.The reaction produces 2 moles of $ \text{AgCl} $ for every 2 moles of $ \text{AgNO}_3 $ reacted. So, the moles of $ \text{AgCl} $ produced are equal to the moles of $ \text{AgNO}_3 $ reacted, which is 0.0600 mol.Finally, we calculate the mass of $ \text{AgCl} $ produced:- Mass of $ \text{AgCl} $ = $ 0.0600 \text{ mol} \times 143.32 \text{ g/mol} $ = 8.60 g, which rounds to 8.61 g when considering significant figures.

Question 6

Balance the following equation. ________ C₁₀H₁₂ + ________ O₂→ ________ H₂O + ________ CO₂

Accepted Answer

The answer of Balance the following equation. ________ C₁₀H₁₂ + ________...

Question 7

Which substance is the limiting reactant when 8.0 g of sulfur reacts with 12 g of oxygen and 16 g of sodium hydroxide according to the following chemical equation: 2 S(s)+ 3 O₂(g)+ 4 NaOH(aq)→ 2 Na₂SO₄(aq)+ 2 H₂O(l)

Accepted Answer

To determine the limiting reactant, we first need to calculate the moles of each reactant. The molar masses are approximately 32 g/mol for sulfur (S), 32 g/mol for oxygen (O2), and 40 g/mol for sodium hydroxide (NaOH). Thus, we have:- 8.0 g S / 32 g/mol = 0.25 mol S- 12 g O2 / 32 g/mol = 0.375 mol O2- 16 g NaOH / 40 g/mol = 0.4 mol NaOHAccording to the stoichiometry of the given reaction, 2 moles of S react with 3 moles of O2 and 4 moles of NaOH. Therefore, for 0.25 moles of S, we would need 0.375 moles of O2 and 0.5 moles of NaOH. Since we only have 0.4 moles of NaOH, which is less than the required 0.5 moles, NaOH is the limiting reactant.

Question 8

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+  (g)→  N(s)
In a particular experiment,1.00-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...

Question 9

If the percent yield for the following reaction is 75.0%,and 25.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq)are produced? 3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

Accepted Answer

First, calculate the theoretical yield of HNO3. The molar mass of NO2 is 46.01 g/mol, and the molar mass of HNO3 is 63.01 g/mol. From the balanced equation, 3 moles of NO2 produce 2 moles of HNO3. Convert 25.0 g of NO2 to moles: 25.0 g / 46.01 g/mol = 0.543 moles of NO2. Using the stoichiometry of the reaction, 0.543 moles NO2 * (2 moles HNO3 / 3 moles NO2) = 0.362 moles HNO3. Convert moles of HNO3 to grams: 0.362 moles * 63.01 g/mol = 22.8 g (theoretical yield). With a 75% yield, the actual yield is 22.8 g * 0.75 = 17.1 g.

Question 10

8.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N₂(g)+ 3 H₂(g)→ 2 NH₃(g)

Accepted Answer

The theoretical yield of ammonia is not 15 g. The correct theoretical yield is calculated using stoichiometry and is approximately 9.8 g.

Question 11

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

Accepted Answer

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

Question 12

9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s)+ 4 H₂O(l)→ Fe₃O₄(s)+ 4 H₂(g)

Accepted Answer

To determine the limiting reactant, we need to calculate the amount of product each reactant can produce. Using the given masses, we can calculate the moles of each reactant: 
moles of Fe = 9.0 g / 55.85 g/mol = 0.161 moles 
moles of H2O = 9.0 g / 18.015 g/mol = 0.499 moles

Using the balanced equation, we can determine that 3 moles of Fe react with 4 moles of H2O to produce 1 mole of FeS13O4. Therefore, the amount of product that can be formed from the available reactants is:

- Fe: 0.161 moles Fe x (1 mol FeS13O4 / 3 mol Fe) = 0.0537 moles FeS13O4
- H2O: 0.499 moles H2O x (1 mol FeS13O4 / 4 mol H2O) = 0.125 moles FeS13O4

Since Fe can only produce 0.0537 moles of product while H2O can produce 0.125 moles, H2O is the limiting reactant. This means that Fe is in excess and there will be some Fe left over after the reaction is complete.

Using the amount of limiting reactant (0.499 moles H2O) and the stoichiometry of the balanced equation, we can calculate the theoretical yield of FeS13O4:

- 0.499 moles H2O x (1 mol FeS13O4 / 4 mol H2O) x 232.14 g/mol = 29.2 g FeS13O4

Therefore, the correct answer is D) Water is the limiting reactant. Statement A is true based on the stoichiometry of the equation and the amount of excess Fe can be calculated using the same approach as above. Statement B is false because all of the H2O is consumed in the reaction. Statement C is true because mass is always conserved in a chemical reaction.

Question 13

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+  O(l)→  (s)
A 5.00-g sample of CaO is reacted with 4.83 g of  O.How many grams of water remain after the reaction is complete?

Accepted Answer

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

Question 14

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+  O(l)→  (s)
In a particular experiment,a 5.50-g sample of CaO is reacted with excess water and 6.77 g of  is recovered.What is the percent yield in this experiment?

Accepted Answer

To calculate the percent yield, we need to use the actual yield (what was recovered in the experiment) and the theoretical yield (what we would expect to get based on stoichiometry), and use the formula: percent yield = (actual yield/theoretical yield) x 100%.

First, we need to calculate the theoretical yield of calcium hydroxide. The balanced equation tells us that for every 1 mole of CaO, we should get 1 mole of Ca(OH)2. The molar mass of CaO is 56.08 g/mol, so the number of moles of CaO in 5.50 g is:

5.50 g CaO x (1 mol CaO/56.08 g CaO) = 0.0981 mol CaO

Therefore, the theoretical yield of Ca(OH)2 is also 0.0981 mol. The molar mass of Ca(OH)2 is 74.09 g/mol, so the theoretical yield in grams is:

0.0981 mol Ca(OH)2 x (74.09 g Ca(OH)2/mol) = 7.27 g Ca(OH)2

Now we can calculate the percent yield:

percent yield = (actual yield/theoretical yield) x 100%
percent yield = (6.77 g/7.27 g) x 100%
percent yield = 93.1%

Therefore, the percent yield is 93.1%, which is choice D.

Question 15

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+  (g)→ 2MgO(s)
When 3.00 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 16

Balance the following equation. ________ C₉H₂₀+ ________ O₂→ ________ H₂O + ________ CO₂

Accepted Answer

The answer of Balance the following equation. ________ C₉H₂₀+ ________...

Question 17

Define a limiting reagent.

Accepted Answer

The answer of Define a limiting reagent....

Question 18

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g)+ 3 O₂(g)→ 2 N₂(g)+ 6 H₂O(g)

Accepted Answer

The answer of When 8.00 × 10²² molecules of ammonia...

Question 19

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 g of O₂? 2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g)

Accepted Answer

The answer of If the percent yield for the following...

Quiz 8: Chemical Reactions and Chemical Quantities

Determine the theoretical yield of H₂S (in moles) if 16 mol Al₂S₃ and 16 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃= 150.17 g/mol. Al₂S₃(s) + 6 H₂O(l) → 2 Al(OH) ₃(s) + 3 H₂S(g)

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

When 14.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + H₂(g)

Describe the greenhouse effect.

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Balance the following equation. C₁₀H₁₂ + O₂→ H₂O + CO₂

Which substance is the limiting reactant when 8.0 g of sulfur reacts with 12 g of oxygen and 16 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O₂(g) + 4 NaOH(aq) → 2 Na₂SO₄(aq) + 2 H₂O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + (g) → N(s) In a particular experiment,1.00-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

If the percent yield for the following reaction is 75.0%,and 25.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq) are produced? 3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

8.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N₂(g) + 3 H₂(g) → 2 NH₃(g)

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

9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s) + 4 H₂O(l) → Fe₃O₄(s) + 4 H₂(g)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + O(l) → (s) A 5.00-g sample of CaO is reacted with 4.83 g of O.How many grams of water remain after the reaction is complete?

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + O(l) → (s) In a particular experiment,a 5.50-g sample of CaO is reacted with excess water and 6.77 g of is recovered.What is the percent yield in this experiment?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + (g) → 2MgO(s) When 3.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Balance the following equation. C₉H₂₀+ O₂→ H₂O + CO₂

Define a limiting reagent.

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g) + 3 O₂(g) → 2 N₂(g) + 6 H₂O(g)

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Quiz 8: Chemical Reactions and Chemical Quantities

Determine the theoretical yield of H2S (in moles) if 16 mol Al2S3 and 16 mol H2O are reacted according to the following balanced reaction.A possibly useful molar mass is Al2S3 = 150.17 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH) 3(s) + 3 H2S(g)

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

When 14.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH) 2(aq) + H2(g)

Describe the greenhouse effect.

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Balance the following equation. ________ C10H12 + ________ O2 → ________ H2O + ________ CO2

Which substance is the limiting reactant when 8.0 g of sulfur reacts with 12 g of oxygen and 16 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na2SO4(aq) + 2 H2O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + (g) → N(s) In a particular experiment,1.00-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

If the percent yield for the following reaction is 75.0%,and 25.0 g of NO2 are consumed in the reaction,how many grams of nitric acid,HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

8.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N2(g) + 3 H2(g) → 2 NH3(g)

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

9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + O(l) → (s) A 5.00-g sample of CaO is reacted with 4.83 g of O.How many grams of water remain after the reaction is complete?

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + O(l) → (s) In a particular experiment,a 5.50-g sample of CaO is reacted with excess water and 6.77 g of is recovered.What is the percent yield in this experiment?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + (g) → 2MgO(s) When 3.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Balance the following equation. ________ C9H20 + ________ O2 → ________ H2O + ________ CO2

Define a limiting reagent.

When 8.00 × 1022 molecules of ammonia react with 7.00 × 1022 molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g)

If the percent yield for the following reaction is 65.0%,how many grams of KClO3 are needed to produce 42.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

Determine the theoretical yield of H₂S (in moles) if 16 mol Al₂S₃ and 16 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃= 150.17 g/mol. Al₂S₃(s) + 6 H₂O(l) → 2 Al(OH) ₃(s) + 3 H₂S(g)

When 14.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + H₂(g)

Balance the following equation. C₁₀H₁₂ + O₂→ H₂O + CO₂

Which substance is the limiting reactant when 8.0 g of sulfur reacts with 12 g of oxygen and 16 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O₂(g) + 4 NaOH(aq) → 2 Na₂SO₄(aq) + 2 H₂O(l)

If the percent yield for the following reaction is 75.0%,and 25.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq) are produced? 3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

8.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N₂(g) + 3 H₂(g) → 2 NH₃(g)

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

9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s) + 4 H₂O(l) → Fe₃O₄(s) + 4 H₂(g)

Balance the following equation. C₉H₂₀+ O₂→ H₂O + CO₂

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g) + 3 O₂(g) → 2 N₂(g) + 6 H₂O(g)

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)