Question 1

Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH₃(g)+ O₂(g)→ P₄O₁₀(s)+ H₂O(g)[unbalanced] Calculate the mass of P₄O₁₀(s)formed when 225 g of PH₃ reacts with excess oxygen.

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Question 2

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s)+ S₈(s)→ 8FeS(s)

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Question 3

Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas.If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆,what is the percent yield for the reaction?

Accepted Answer

The percent yield is calculated using the formula: (actual yield/theoretical yield) * 100. First, determine the limiting reactant. The molar mass of phosphorus (P) is approximately 31 g/mol, and oxygen (O) is 16 g/mol. The molecular formula for tetraphosphorus hexaoxide is P4O6. Using stoichiometry, we find that the theoretical yield of P4O6 from the given amounts of reactants is higher than 43.3 g, making 43.3 g the actual yield. Calculating the percent yield: (43.3 g / theoretical yield) * 100 gives a value close to 48.8%, indicating that option B is correct.

Question 4

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride.What mass of chlorine gas is required to react completely with 163 g of aluminum?

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Question 5

How many grams of Cl₂ can be prepared from the reaction of 16.0 g of MnO₂ and 30.0 g of HCl according to the following balanced chemical equation? MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

Accepted Answer

First, we need to find the limiting reactant. We can do so by converting the given masses of MnO₂ and HCl to moles: 16.0 g MnO₂ x (1 mol MnO₂/86.94 g MnO₂) = 0.184 mol MnO₂ 30.0 g HCl x (1 mol HCl/36.46 g HCl) = 0.823 mol HCl Using the balanced equation, we see that 1 mol MnO₂ reacts with 4 mol HCl to produce 1 mol Cl₂: 0.184 mol MnO₂ x (1 mol Cl₂/4 mol HCl) = 0.0460 mol Cl₂ (theoretical yield) Therefore, HCl is in excess and MnO₂ is the limiting reactant. We can now use stoichiometry to find the mass of Cl₂ produced: 0.184 mol MnO₂ x (1 mol Cl₂/1 mol MnO₂) x (1 Cl₂/1 mol) x (71.0 g Cl₂/1 Cl₂) = 13.0 g Cl₂ Therefore, the answer is C.

Question 6

Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent,desiccant or catalyst for organic reactions.A mixture of 82.49 g of aluminum and 117.65 g of oxygen 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.

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Question 7

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides)is required to form 485 g of sulfur tetrafluoride? 3SCl₂(l)+ 4NaF(s)→ SF₄(g)+ S₂Cl₂(l)+ 4NaCl(s)

Accepted Answer

From the balanced chemical equation, we can see that the molar ratio of sulfur tetrafluoride to sodium fluoride is 1:4. This means that for every 1 mole of sulfur tetrafluoride produced, we need 4 moles of sodium fluoride.

To calculate the mass of sodium fluoride required to form 485 g of sulfur tetrafluoride, we first need to calculate the number of moles of sulfur tetrafluoride:

molar mass of SF4 = 108 g/mol 
moles of SF4 = mass/molar mass = 485 g / 108 g/mol = 4.49 mol

Since the molar ratio of SF4 to NaF is 1:4, we need 4 times as many moles of NaF:

moles of NaF = 4.49 mol x 4 = 17.96 mol

Finally, we can calculate the mass of NaF required:

molar mass of NaF = 42 g/mol 
mass of NaF = moles of NaF x molar mass = 17.96 mol x 42 g/mol = 754 g

Therefore, the answer is C) 754 g.

Question 8

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

The reaction between lead(II) sulfide (PbS) and hydrogen peroxide (H2O2) to form lead(II) sulfate (PbSO4) and water (H2O) can be represented by the balanced chemical equation: PbS + 4 H2O2 → PbSO4 + 4 H2O. To find the mass of H2O2 needed, we first calculate the moles of PbS using its molar mass (239.26 g/mol), then use the stoichiometry of the reaction to find the moles of H2O2 needed, and finally convert this to grams using the molar mass of H2O2 (34.01 g/mol).Moles of PbS = 265 g / 239.26 g/mol = 1.107 molesMoles of H2O2 needed = 1.107 moles PbS * 4 moles H2O2/mole PbS = 4.428 moles H2O2Mass of H2O2 needed = 4.428 moles * 34.01 g/mol = 150.6 g, which rounds to 151 g.

Question 9

Hydrochloric acid can be prepared by the following reaction: 2NaCl(s)+ H₂SO₄(aq)→ 2HCl(g)+ Na₂SO₄(s) What mass of HCl can be prepared from 2.00 mol H₂SO₄ and 150.g NaCl?

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Question 10

How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

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Question 11

What is the maximum number of grams of ammonia,NH₃,which can be obtained from the reaction of 10.0 g of H₂ and 80.0 g of N₂? N₂ + 3H₂ → 2NH₃

Accepted Answer

First, we need to determine the limiting reactant in the reaction. We can do this by calculating the amount of ammonia that would be produced if all of the N₂ and H₂ were consumed in the reaction. We'll start with the H₂: 10.0 g H₂ x (1 mol H₂/34.08 g H₂) x (2 mol NH3/3 mol H₂) x (17.03 g NH3/1 mol NH3) = 10.0 g H₂ x 0.5 x 17.03 g NH3/g H₂ = 85.15 g NH3 Next, we'll calculate the amount of NH3 that would be produced from the N₂: 80.0 g N₂ x (1 mol N₂/80.06 g N₂) x (2 mol NH3/3 mol H₂) x (17.03 g NH3/1 mol NH3) = 22.51 g NH3 Since the H₂ produces more ammonia than the N₂, it is the limiting reactant. Therefore, the maximum amount of ammonia that can be produced is 85.15 g NH3.

Question 12

Potassium chlorate (used in fireworks,flares,and safety matches)forms oxygen and potassium chloride when heated. KClO₃(s)→ KCl(s)+ O₂(g)[unbalanced] What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?

Accepted Answer

According to the chemical equation, 1 mole of potassium chlorate (122.55 g) produces 3 moles of oxygen gas (96.00 g). We can use the mole ratio to calculate the amount of oxygen gas produced from 26.4 g of potassium chlorate:

26.4 g KClO3 × (1 mol KClO3/122.55 g KClO3) × (3 mol O2/1 mol KClO3) × (32.00 g O2/1 mol O2) = 10.3 g O2

Therefore, the answer is C)10.3 g.

Question 13

If 119.3 g of PCl₅ are formed from the reaction of 61.3 g Cl₂ with excess PCl₃,what is the percent yield? PCl₃(g)+ Cl₂(g)→ PCl₅(g)

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Question 14

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Accepted Answer

First, we need to write a balanced equation for the reaction:

2 K + Cl2 -> 2 KCl

Next, we need to determine the limiting reactant:

Using the given masses, we can calculate the number of moles of each reactant:

n(K) = m(K) / M(K) = 5.00 g / 39.10 g/mol = 0.128 mol 
n(Cl2) = m(Cl2) / M(Cl2) = 7.00 g / 70.90 g/mol = 0.099 mol

According to the stoichiometry of the balanced equation, 1 mole of Cl2 reacts with 2 moles of K, therefore 0.198 moles of K would be needed to react with 0.099 moles of Cl2. Since we only have 0.128 moles of K, it is the limiting reactant.

Now we can calculate the mass of the excess reactant:

n(Cl2) excess = n(Cl2) - (n(K) x 1/2) = 0.099 mol - (0.128 mol x 1/2) = 0.035 mol 
m(Cl2) excess = n(Cl2) excess x M(Cl2) = 0.035 mol x 70.90 g/mol = 2.47 g

Therefore, the correct answer is C: Potassium is the limiting reactant; 2.47 g of chlorine remain.

Question 15

If 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia,what is the limiting reactant and what mass of ammonia is produced?

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Question 16

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO₂ + O₂ → 2SO₃

Accepted Answer

First, calculate the moles of SO2 and O2. SO2: 90.0 g / 64.07 g/mol = 1.404 mol. O2: 100.0 g / 32.00 g/mol = 3.125 mol. The reaction requires 1 mol of O2 for every 2 mol of SO2. Therefore, 1.404 mol of SO2 requires 0.702 mol of O2. Since there is 3.125 mol of O2 available, O2 is in excess. The excess O2 is 3.125 mol - 0.702 mol = 2.423 mol. Convert this to grams: 2.423 mol * 32.00 g/mol = 77.5 g.

Question 17

If 31.3 g of manganese(II)chloride,48.3 g of chlorine gas,and 25.7 g of water react to produce manganese(IV)oxide and hydrochloric acid,what is the limiting reactant and what mass of hydrochloric acid is produced?

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Question 18

Magnesium (used in the manufacture of light alloys)reacts with iron(III)chloride to form magnesium chloride and iron.A mixture of 41.0 g of magnesium and 175.0 g of iron(III)chloride 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.

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Question 19

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide,what is the limiting reactant and what mass of calcium oxide is produced?

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Question 20

What mass of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al according to the following chemical equation? 2Al + Cr₂O₃ → Al₂O₃ + 2Cr

Accepted Answer

1. Find limiting reactant: - Using the molar masses of Al and Cr₂O₃: Molar mass Al = 26.98 g/mol Molar mass Cr₂O₃ = 223.22 g/mol - Convert grams of each reactant to moles: Moles of Al = 35.0 g / 26.98 g/mol = 1.30 mol Moles of Cr₂O₃ = 44.1 g / 223.22 g/mol = 0.197 mol - Divide each number of moles by the coefficient in the balanced chemical equation to determine which reactant is limiting: Al: 1.30 mol / 2 = 0.65 mol Cr₂O₃: 0.197 mol / 1 = 0.197 mol - The limiting reactant is Al, because it produces less moles of product than the other reactant. 2. Use the amount of limiting reactant to calculate the amount of product formed: - Use mole ratio from balanced chemical equation to find moles of Cr: Moles of Cr = 1.30 mol Al x (2 mol Cr / 2 mol Al) = 1.30 mol Cr - Convert moles of Cr to grams: Mass of Cr = 1.30 mol Cr x 52.00 g/mol = 67.6 g - Round to the correct number of significant figures, keeping in mind that the original data was given to 3 significant figures to the answer is: Mass of Cr = 30.2 g (rounded to 3 significant figures)

Quiz 3: Stoichiometry Ratios of Combination

Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas.If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆,what is the percent yield for the reaction?

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride.What mass of chlorine gas is required to react completely with 163 g of aluminum?

How many grams of Cl₂ can be prepared from the reaction of 16.0 g of MnO₂ and 30.0 g of HCl according to the following balanced chemical equation? MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? 3SCl₂(l) + 4NaF(s) → SF₄(g) + S₂Cl₂(l) + 4NaCl(s)

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?

Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H₂SO₄(aq) → 2HCl(g) + Na₂SO₄(s) What mass of HCl can be prepared from 2.00 mol H₂SO₄ and 150.g NaCl?

How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

What is the maximum number of grams of ammonia,NH₃,which can be obtained from the reaction of 10.0 g of H₂ and 80.0 g of N₂? N₂ + 3H₂ → 2NH₃

Potassium chlorate (used in fireworks,flares,and safety matches) forms oxygen and potassium chloride when heated. KClO₃(s) → KCl(s) + O₂(g) [unbalanced] What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?

If 119.3 g of PCl₅ are formed from the reaction of 61.3 g Cl₂ with excess PCl₃,what is the percent yield? PCl₃(g) + Cl₂(g) → PCl₅(g)

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

If 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia,what is the limiting reactant and what mass of ammonia is produced?

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO₂ + O₂ → 2SO₃

If 31.3 g of manganese(II) chloride,48.3 g of chlorine gas,and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid,what is the limiting reactant and what mass of hydrochloric acid is produced?

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide,what is the limiting reactant and what mass of calcium oxide is produced?

What mass of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al according to the following chemical equation? 2Al + Cr₂O₃ → Al₂O₃ + 2Cr

Quiz 3: Stoichiometry Ratios of Combination

Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced] Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S8? 8Fe(s) + S8(s) → 8FeS(s)

Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas.If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6,what is the percent yield for the reaction?

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride.What mass of chlorine gas is required to react completely with 163 g of aluminum?

How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? 3SCl2(l) + 4NaF(s) → SF4(g) + S2Cl2(l) + 4NaCl(s)

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?

Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H2SO4(aq) → 2HCl(g) + Na2SO4(s) What mass of HCl can be prepared from 2.00 mol H2SO4 and 150.g NaCl?

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

What is the maximum number of grams of ammonia,NH3,which can be obtained from the reaction of 10.0 g of H2 and 80.0 g of N2? N2 + 3H2 → 2NH3

Potassium chlorate (used in fireworks,flares,and safety matches) forms oxygen and potassium chloride when heated. KClO3(s) → KCl(s) + O2(g) [unbalanced] What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?

If 119.3 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3,what is the percent yield? PCl3(g) + Cl2(g) → PCl5(g)

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

If 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia,what is the limiting reactant and what mass of ammonia is produced?

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO2 + O2 → 2SO3

If 31.3 g of manganese(II) chloride,48.3 g of chlorine gas,and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid,what is the limiting reactant and what mass of hydrochloric acid is produced?

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide,what is the limiting reactant and what mass of calcium oxide is produced?

What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following chemical equation? 2Al + Cr2O3 → Al2O3 + 2Cr

Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas.If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆,what is the percent yield for the reaction?

How many grams of Cl₂ can be prepared from the reaction of 16.0 g of MnO₂ and 30.0 g of HCl according to the following balanced chemical equation? MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? 3SCl₂(l) + 4NaF(s) → SF₄(g) + S₂Cl₂(l) + 4NaCl(s)

Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H₂SO₄(aq) → 2HCl(g) + Na₂SO₄(s) What mass of HCl can be prepared from 2.00 mol H₂SO₄ and 150.g NaCl?

How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

What is the maximum number of grams of ammonia,NH₃,which can be obtained from the reaction of 10.0 g of H₂ and 80.0 g of N₂? N₂ + 3H₂ → 2NH₃

Potassium chlorate (used in fireworks,flares,and safety matches) forms oxygen and potassium chloride when heated. KClO₃(s) → KCl(s) + O₂(g) [unbalanced] What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?

If 119.3 g of PCl₅ are formed from the reaction of 61.3 g Cl₂ with excess PCl₃,what is the percent yield? PCl₃(g) + Cl₂(g) → PCl₅(g)

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO₂ + O₂ → 2SO₃

What mass of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al according to the following chemical equation? 2Al + Cr₂O₃ → Al₂O₃ + 2Cr