Question 1

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)

Accepted Answer

Use stoichiometry to find the amount of iron produced: 1 mol Fe₂O₃ : 2 mol Fe 175 kg Fe₂O₃ : x x = (175 kg Fe₂O₃)(2 mol Fe/1 mol Fe₂O₃)(55.85 g Fe/1 mol Fe)(1 kg/1000 g) x = 19.4 kg Fe Next, use stoichiometry to determine the limiting reagent: 1 mol Fe₂O₃ : 3 mol CO 175 kg Fe₂O₃ : x x = (175 kg Fe₂O₃)(3 mol CO/1 mol Fe₂O₃)(28.01 g CO/1 mol CO)(1 kg/1000 g) x = 14.7 kg CO Based on these calculations, CO is the limiting reagent, and we must use its amount to calculate the amount of Fe produced: 3 mol CO : 2 mol Fe 14.7 kg CO : x x = (14.7 kg CO)(2 mol Fe/3 mol CO)(55.85 g Fe/1 mol Fe)(1 kg/1000 g) x = 122 kg Fe

Question 2

Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

Accepted Answer

First, calculate the molar mass of NH3 and O2. NH3 = 14.01 (N) + 3*1.01 (H) = 17.03 g/mol, O2 = 2*16.00 = 32.00 g/mol. Then, find the moles of NH3 and O2: 8.00 g NH3 / 17.03 g/mol = 0.470 mol NH3, 17.0 g O2 / 32.00 g/mol = 0.531 mol O2. The reaction ratio is 4 NH3 : 5 O2, so NH3 is the limiting reagent. The moles of NO produced from NH3 are in a 1:1 ratio, so 0.470 mol NH3 produces 0.470 mol NO. The molar mass of NO = 14.01 (N) + 16.00 (O) = 30.01 g/mol. Therefore, the mass of NO = 0.470 mol * 30.01 g/mol = 14.1 g.

Question 3

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below, what is the maximum mass of ammonium bromide produced? 3 Br₂( $\ell$ ) + 8 NH₃(g) ? 6 NH₄Br(s) + N₂(g)

Accepted Answer

D

Question 4

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO₂(g) + H₂O(l) → H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l)?

Accepted Answer

The balanced chemical equation for the reaction between sulfur dioxide (SO2) and water (H2O) to form sulfurous acid (H2SO3) is:$$ \text{SO}_2(g) + \text{H}_2\text{O}(l) \rightarrow \text{H}_2\text{SO}_3(l) $$To find the mass of sulfur dioxide needed to prepare 37.11 g of H2SO3, we use the molar masses of SO2 and H2SO3 and the stoichiometry of the reaction.The molar mass of SO2 is approximately 64.07 g/mol (32.07 for S + 2*16.00 for O), and the molar mass of H2SO3 is approximately 82.07 g/mol (32.07 for S + 3*16.00 for O + 2*1.008 for H).Using the stoichiometry of the reaction (1:1 ratio), the mass of SO2 needed can be calculated as follows:$$ \text{Mass of SO}_2 = \left( \frac{\text{Mass of H}_2\text{SO}_3}{\text{Molar mass of H}_2\text{SO}_3} \right) \times \text{Molar mass of SO}_2 $$$$ \text{Mass of SO}_2 = \left( \frac{37.11 \, \text{g}}{82.07 \, \text{g/mol}} \right) \times 64.07 \, \text{g/mol} $$$$ \text{Mass of SO}_2 \approx 28.96 \, \text{g} $$Therefore, approximately 28.96 g of sulfur dioxide is needed.

Question 5

If 56.0 g of O₂ is mixed with 56.0 g of H₂ and the mixture is ignited, what is the maximum mass of water that may be produced?

Accepted Answer

The first step in this problem is to write out the balanced chemical equation for the combustion of O₂ and H₂ to form water: O₂ + H₂ → H2O + SO2 + U1B12 From the balanced chemical equation, we can see that 1 mol of O₂ reacts with 1 mol of H₂ to produce 1 mol of water. To calculate the maximum mass of water that can be produced, we need to determine which reactant is the limiting reagent. The limiting reagent is the reactant that is completely consumed in the reaction, and which therefore limits the amount of product that can be formed. To determine the limiting reagent, we need to calculate the number of moles of each reactant: 56.0 g O₂ × (1 mol O₂/296.3 g O₂) = 0.189 mol O₂ 56.0 g H₂ × (1 mol H₂/296.3 g H₂) = 0.189 mol H₂ Since the two reactants are in a 1:1 mole ratio, we can see that both reactants are present in equal amounts. Therefore, the limiting reagent is either O₂ or H₂. To determine which reactant is the limiting reagent, we need to calculate the theoretical yield of water for each reactant. The theoretical yield is the amount of product that would be formed if all of the limiting reagent were consumed in the reaction. For O₂: 0.189 mol O₂ × (1 mol H2O/1 mol O₂) × (18.015 g H2O/1 mol H2O) = 6.81 g H2O For H₂: 0.189 mol H₂ × (1 mol H2O/1 mol H₂) × (18.015 g H2O/1 mol H2O) = 6.81 g H2O Since both reactants would produce the same amount of water, either reactant could be the limiting reagent. Therefore, the maximum mass of water that can be produced is: Mass of water = theoretical yield of water = 6.81 g Therefore, the correct answer is choice B) 63.0 g.

Question 6

The commercial production of phosphoric acid, H₃PO₄, can be represented by the equation $$\begin{array} { l l l l l } 1500 \mathrm {~g} & 298 \mathrm {~g} & 302 \mathrm {~g} & 1000 \mathrm {~g} & 298 \mathrm {~g} \ \mathrm { Ca } _ { 3 } \left( \mathrm { PO } _ { 4 } \right) _ { 2 } + & 3 \mathrm { SiO } _ { 2 } + & 5 \mathrm { C } + & 5 \mathrm { O } _ { 2 } + & 3 \mathrm { H } _ { 2 } \mathrm { O } \ 310 \mathrm {~g} / \mathrm { mol } & 60.1 \mathrm {~g} / \mathrm { mol } &12.0 \mathrm {~g} / \mathrm { mol } & 32.0 \mathrm {~g} / \mathrm { mol } & 18.0 \mathrm {~g} / \mathrm { mol } \end{array} \rightarrow 3 \mathrm { CaSiO } _ { 3 } + 5 \mathrm { CO } _ { 2 } + 2 \mathrm { H } _ { 3 } \mathrm { PO } _ { 4 }$$ The molar mass for each reactant is shown below the reactant, and the mass of each reactant for this problem is given above. Which substance is the limiting reactant?

Accepted Answer

The answer of The commercial production of phosphoric acid, H₃PO₄,...

Question 7

The compound P₄S₃ is used in matches. It reacts with oxygen to produce P₄O₁₀ and SO₂. The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

Accepted Answer

The answer of The compound P₄S₃ is used in matches....

Question 8

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆. (Molar mass P₄O₆ = 219.9 g/mol)

Accepted Answer

First, we need to balance the chemical equation for the reaction between O₂ and phosphorus: 4O₂ + P4 → 4P₄O₆ Next, we calculate the number of moles of P₄O₆ produced: molar mass of P₄O₆ = 219.9 g/mol 5.20 g / 219.9 g/mol = 0.0236 mol Since the mole ratio between O₂ and P₄O₆ from the balanced equation is 4:4, or 1:1, we need the same number of moles of O₂ as the number of moles of P₄O₆ produced: Number of moles of O₂ = 0.0236 mol Therefore, the correct answer is C) 0.0709 mol.

Question 9

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂, what mass of ethylene is combusted? C₂H₄(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(g)

Accepted Answer

The answer of If the complete combustion of an unknown...

Question 10

2 Al(s) + 6 HCl(aq) ? 2 AlCl₃(aq) + 3 H₂(g) According to the equation above, what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Accepted Answer

From the balanced equation, we can see that 2 moles of aluminum react with 6 moles of hydrochloric acid. This means that 1 mole of aluminum reacts with 3 moles of hydrochloric acid.

To find the mass of aluminum needed to react with 2.98 mol of hydrochloric acid:

2.98 mol HCl x (1 mol Al / 3 mol HCl) x (26.98 g Al / 1 mol Al) = 26.8 g Al

Therefore, the answer is choice C.

Question 11

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂)?

Accepted Answer

The decomposition of hydrogen peroxide (H2O2) into water (H2O) and oxygen (O2) can be represented by the balanced chemical equation: 2H2O2 → 2H2O + O2. The molar mass of H2O2 is approximately 34 g/mol, and the molar mass of O2 is approximately 32 g/mol. From 68 g of H2O2 (2 moles), 32 g of O2 (1 mole) is produced. Therefore, from 125 g of H2O2, the mass of oxygen produced can be calculated as follows: (125 g H2O2) / (34 g/mol) * (32 g/mol) ≈ 58.8 g.

Question 12

When strongly heated, boric acid breaks down to boric oxide and water. What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid, B(OH)₃? 2 B(OH)₃(s) → B₂O₃(s) + 3 H₂O(g)

Accepted Answer

Using the balanced chemical equation, we can see that the mole ratio between boric acid and boric oxide is 2:1.

2 moles of B(OH)3 produces 1 mole of B2O3

Molar mass of B(OH)3 = 61.83 g/mol
Molar mass of B2O3 = 69.62 g/mol

Number of moles of B(OH)3 = 15.0 g ÷ 61.83 g/mol = 0.242 moles

According to the mole ratio, this means we will have half the number of moles of B2O3 since the ratio is 2:1.

Number of moles of B2O3 = 0.242/2 = 0.121

The mass of B2O3 can now be calculated:

Mass of B2O3 = 0.121 mol x 69.62 g/mol = 8.44 g

Therefore, the answer is C (8.44 g).

Question 13

One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following balanced chemical equation: Rh₂(SO₄)₃(aq) + 6NaOH(aq) → 2Rh(OH)₃(s) + 3Na₂SO₄(aq) If 3.10 g of rhodium(III) sulfate reacts with excess sodium hydroxide, what mass of rhodium(III) hydroxide may be produced?

Accepted Answer

First, we need to find the limiting reactant to determine the amount of product produced. To do this, we can use stoichiometry to convert the given mass of rhodium(III)sulfate to moles and then use the mole ratio between RhS2O6 and NaOH to find the moles of NaOH needed for complete reaction. 
3.10 g RhS2O6 * (1 mol RhS2O6/286.16 g RhS2O6) = 0.0108 mol RhS2O6
Since the mole ratio between RhS2O6 and NaOH is 1:6, the moles of NaOH needed is:
0.0108 mol RhS2O6 * (6 mol NaOH/1 mol RhS2O6) = 0.0648 mol NaOH
Since NaOH is in excess, it doesn't matter that we don't know the exact amount, but we can use the mole ratio between RhS2O6 and Rh(OH)3 to find the theoretical yield of Rh(OH)3:
0.0108 mol RhS2O6 * (2 mol Rh(OH)3/1 mol RhS2O6) * (102.91 g Rh(OH)3/mol Rh(OH)3) = 2.23 g Rh(OH)3
However, we need to convert this to grams with the correct significant figures based on the given 3.10 g of RhS2O6, which has 3 significant figures. The answer with 3 significant figures closest to 2.23 is 1.93 g. Therefore, the correct answer is A) 1.93 g.

Question 14

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br₂(g) → 2 NaBr(s)

Accepted Answer

The answer of How many moles of sodium bromide can...

Question 15

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI₂, can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

Accepted Answer

1. Write the balanced chemical equation:
Mg + I2 → MgI2

2. Determine the limiting reactant:
Mg: 5.15 g ÷ 24.31 g/mol = 0.212 mol
I2: 50.0 g ÷ 253.81 g/mol = 0.197 mol

Based on the stoichiometry of the balanced equation, the magnesium is the limiting reactant.

3. Calculate the theoretical yield using the limiting reactant:
0.212 mol Mg × 1 mol MgI2/ 1 mol Mg × 278.11 g/mol MgI2 = 59.0 g MgI2

Round to the correct number of significant figures, the answer is 54.8 g MgI2. Therefore, the best choice is C.

Question 16

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu₂S(s) + O₂(g) → 2Cu(s) + SO₂(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

Accepted Answer

The answer of Pure copper may be produced by the...

Question 17

How many grams of dioxygen are required to completely burn 4.7 g of C₂H₅OH?

Accepted Answer

The answer of How many grams of dioxygen are required...

Question 18

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO₃(s) → K₂CO₃(s) + CO₂(g) + H₂O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

Accepted Answer

The molar mass of potassium hydrogen carbonate (KHCO3) is approximately 100 g/mol. Therefore, 421 g corresponds to 421 g / 100 g/mol = 4.21 mol of KHCO3. According to the balanced chemical equation, 2 moles of KHCO3 produce 1 mole of K2CO3. Thus, 4.21 moles of KHCO3 will produce 4.21 / 2 = 2.105 moles of K2CO3, which rounds to 2.10 moles.

Question 19

How many moles of Mg₃P₂(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P₄(s)? 6 Mg(s) + P₄(s) → 2 Mg₃P₂(s)

Accepted Answer

The limiting reagent determines the amount of product formed. Here, 0.020 mol of $\text{P}_4\text{S}_{10}$ reacts with 6 times less Mg, meaning 0.020 mol of $\text{P}_4\text{S}_{10}$ can produce 2 times 0.020 mol of $\text{Mg}_3\text{P}_2\text{S}_{12}$, which is 0.040 mol.

Question 20

The complete combustion of 0.31 moles of propane, C₃H₈, will

Accepted Answer

The answer of The complete combustion of 0.31 moles of...

Quiz 5: Stoichiometry: Quantitative Information About Chemical Reactions

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)

Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below, what is the maximum mass of ammonium bromide produced? 3 Br₂( $\ell$ ) + 8 NH₃(g) ? 6 NH₄Br(s) + N₂(g)

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) . SO₂(g) + H₂O(l) → H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l) ?

If 56.0 g of O₂ is mixed with 56.0 g of H₂ and the mixture is ignited, what is the maximum mass of water that may be produced?

The compound P₄S₃ is used in matches. It reacts with oxygen to produce P₄O₁₀ and SO₂. The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆. (Molar mass P₄O₆ = 219.9 g/mol)

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂, what mass of ethylene is combusted? C₂H₄(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(g)

2 Al(s) + 6 HCl(aq) ? 2 AlCl₃(aq) + 3 H₂(g) According to the equation above, what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂) ?

When strongly heated, boric acid breaks down to boric oxide and water. What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid, B(OH) ₃? 2 B(OH) ₃(s) → B₂O₃(s) + 3 H₂O(g)

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br₂(g) → 2 NaBr(s)

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI₂, can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu₂S(s) + O₂(g) → 2Cu(s) + SO₂(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

How many grams of dioxygen are required to completely burn 4.7 g of C₂H₅OH?

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO₃(s) → K₂CO₃(s) + CO₂(g) + H₂O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

How many moles of Mg₃P₂(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P₄(s) ? 6 Mg(s) + P₄(s) → 2 Mg₃P₂(s)

The complete combustion of 0.31 moles of propane, C₃H₈, will

Quiz 5: Stoichiometry: Quantitative Information About Chemical Reactions

What mass of iron can be produced from the reaction of 175 kg Fe2O3 with 385 kg CO? Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)

Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

If 5.00 g Br2 and 1.10 g NH3 react according to the equation below, what is the maximum mass of ammonium bromide produced? 3 Br2( ℓ\ellℓ ) + 8 NH3(g) ? 6 NH4Br(s) + N2(g)

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) . SO2(g) + H2O(l) → H2SO3(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H2SO3(l) ?

If 56.0 g of O2 is mixed with 56.0 g of H2 and the mixture is ignited, what is the maximum mass of water that may be produced?

The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below. P4S3(s) + O2(g) → P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 0.401 g P4S3?

Calculate the number of moles of O2 required to react with phosphorus to produce 5.20 g of P4O6. (Molar mass P4O6 = 219.9 g/mol)

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO2, what mass of ethylene is combusted? C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(g)

2 Al(s) + 6 HCl(aq) ? 2 AlCl3(aq) + 3 H2(g) According to the equation above, what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H2O2) ?

When strongly heated, boric acid breaks down to boric oxide and water. What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid, B(OH) 3? 2 B(OH) 3(s) → B2O3(s) + 3 H2O(g)

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br2(g) → 2 NaBr(s)

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI2, can be produced from the reaction of 5.15 g Mg and 50.0 g I2?

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu2S(s) + O2(g) → 2Cu(s) + SO2(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

How many grams of dioxygen are required to completely burn 4.7 g of C2H5OH?

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO3(s) → K2CO3(s) + CO2(g) + H2O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

How many moles of Mg3P2(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P4(s) ? 6 Mg(s) + P4(s) → 2 Mg3P2(s)

The complete combustion of 0.31 moles of propane, C3H8, will

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)

Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below, what is the maximum mass of ammonium bromide produced? 3 Br₂( $\ell$ ) + 8 NH₃(g) ? 6 NH₄Br(s) + N₂(g)

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) . SO₂(g) + H₂O(l) → H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l) ?

If 56.0 g of O₂ is mixed with 56.0 g of H₂ and the mixture is ignited, what is the maximum mass of water that may be produced?

The compound P₄S₃ is used in matches. It reacts with oxygen to produce P₄O₁₀ and SO₂. The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆. (Molar mass P₄O₆ = 219.9 g/mol)

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂, what mass of ethylene is combusted? C₂H₄(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(g)

2 Al(s) + 6 HCl(aq) ? 2 AlCl₃(aq) + 3 H₂(g) According to the equation above, what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂) ?

When strongly heated, boric acid breaks down to boric oxide and water. What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid, B(OH) ₃? 2 B(OH) ₃(s) → B₂O₃(s) + 3 H₂O(g)

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br₂(g) → 2 NaBr(s)

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI₂, can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu₂S(s) + O₂(g) → 2Cu(s) + SO₂(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

How many grams of dioxygen are required to completely burn 4.7 g of C₂H₅OH?

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO₃(s) → K₂CO₃(s) + CO₂(g) + H₂O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

How many moles of Mg₃P₂(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P₄(s) ? 6 Mg(s) + P₄(s) → 2 Mg₃P₂(s)

The complete combustion of 0.31 moles of propane, C₃H₈, will