Question 1

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g). What weight of CO₂ is obtained by the decomposition of 38.7 g of CaCO₃?

Accepted Answer

From the balanced chemical equation, we can see that the mole ratio of CaCO₃ to CO₂ is 1:1. Therefore, we can calculate the number of moles of CaCO₃: 38.7 g CaCO₃ x (1 mol CaCO₃/100.1 g CaCO₃) = 0.386 mol CaCO₃ Since the mole ratio of CaCO₃ to CO₂ is 1:1, the number of moles of CO₂ produced is also 0.386 mol. Finally, we can calculate the weight of CO₂ produced: 0.386 mol CO₂ x (44.01 g CO₂/1 mol CO₂) = 17.0 g CO₂. Therefore, the answer is B.

Question 2

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l) How much Ag₂O is produced when 0.200 g of AgNO₃ and 0.200 g of NaOH react?

Accepted Answer

The answer of When solutions of AgNO₃ and NaOH react,...

Question 3

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g). What weight of elemental mercury will be obtained by the decomposition of 0.125 mol of HgO?

Accepted Answer

The molar mass of HgO is approximately 216.59 g/mol, and the molar mass of Hg is approximately 200.59 g/mol. From the balanced equation, 2 moles of HgO produce 2 moles of Hg. Therefore, 0.125 moles of HgO will produce 0.125 moles of Hg. The weight of 0.125 moles of Hg is 0.125 mol × 200.59 g/mol = 25.07 g, which is closest to 25.0 g.

Question 4

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g). What weight of oxygen is required to completely burn 19.8 g of octane?

Accepted Answer

The answer of The balanced equation for burning octane is:...

Question 5

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l) How much Ag₂O is produced when 2.00 g of AgNO₃ and 0.300 g of NaOH react?

Accepted Answer

1) First, we need to determine the limiting reagent. To do this, we can use stoichiometry and convert the given masses of AgNO₃ and NaOH to moles: - Moles of AgNO₃ = 2.00 g / 169.87 g/mol = 0.01177 mol - Moles of NaOH = 0.300 g / 40.00 g/mol = 0.0075 mol 2) Next, we can use the coefficients of the balanced equation to determine the mole ratio between AgNO₃ and Ag₂O: - 2 moles of AgNO₃ produce 1 mole of Ag₂O (from the balanced equation) 3) Using the mole ratio, we can calculate the theoretical yield of Ag₂O if all of the AgNO₃ reacted: - Theoretical yield of Ag₂O = 0.01177 mol AgNO₃ × (1 mol Ag₂O / 2 mol AgNO₃) × (328.89 g/mol Ag₂O / 1 mol Ag₂O) = 0.992 g 4) However, we know that NaOH is the limiting reagent, since it produces less moles of product than AgNO₃ does. Using stoichiometry, we can calculate how many moles of Ag₂O will be produced by the reaction of all the NaOH: - Moles of Ag₂O = 0.0075 mol NaOH × (1 mol Ag₂O / 2 mol NaOH) = 0.00375 mol 5) Finally, we can convert the moles of Ag₂O to grams: - Mass of Ag₂O = 0.00375 mol × (328.89 g/mol) = 1.236 g Since we are looking for the actual yield of Ag₂O, which is the amount produced in the reaction, we will take the smaller value between the theoretical yield (0.992 g) and the yield calculated using the limiting reagent (1.236 g). Therefore, the answer is A) 0.869 g, which is the amount of Ag₂O that can actually be produced based on the given reactant quantities.

Question 6

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 160 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

Accepted Answer

To manufacture a bicycle, we need one frame and two wheels, thus we can assemble `(70/2 = 35)` 35 bicycles with 70 wheels. Now since each bicycle requires 4 reflectors, we need a total of `(35 * 4 = 140)` 140 reflectors to assemble 35 bicycles. But we only have 160 reflectors, which means we can manufacture only `(160 / 4 = 40)` 40 bicycles (using 160 reflectors and 40 frames).

Question 7

In a particular experiment to prepare a compound, the theoretical yield is 34.7 G) If the actual yield is 31.2 g, what is the percent yield?

Accepted Answer

Percent yield = (actual yield/theoretical yield) x 100%
Percent yield = (31.2/34.7) x 100% = 89.9%

Question 8

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 120 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

Accepted Answer

To make a bicycle, we need one frame and two wheels. As there are only 50 frames, we can make a maximum of 50 bicycles. However, we also need 4 reflectors per bicycle, which means we need a total of 50 x 4 = 200 reflectors. But the manufacturer only has 120 reflectors, which is not enough to make 50 bicycles. Therefore, the maximum number of bicycles that can be made is limited by the number of reflectors available. Since we have 120 reflectors, we can make a maximum of 120/4 = 30 bicycles. The correct choice is B.

Question 9

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 0.600 g of NaCl react?

Accepted Answer

The limiting reactant is AgNO3. Moles of AgNO3 = 3.10 g / 169.87 g/mol = 0.0182 mol. Moles of NaCl = 0.600 g / 58.44 g/mol = 0.0103 mol. AgNO3 is in excess. Moles of AgCl produced = 0.0103 mol. Mass of AgCl = 0.0103 mol * 143.32 g/mol = 1.47 g.

Question 10

In an experiment to prepare aspirin, the percent yield was 94.3% G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

Accepted Answer

The percent yield is calculated as (actual yield/theoretical yield) x 100. Rearranging to find the theoretical yield gives theoretical yield = actual yield / (percent yield/100). Substituting the given values: theoretical yield = 124.3 g / (94.3/100) = 131.8 g, which rounds to 132 g.

Question 11

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) What weight of H₂O is produced by completely burning 19.8 g of octane?

Accepted Answer

The balanced equation shows that 2 moles of octane produce 18 moles of water. The molar mass of octane is 114.23 g/mol, so 19.8 g of octane is 0.173 mol. This will produce 0.173 mol * 18 mol/2 mol = 1.55 mol of water. The molar mass of water is 18.02 g/mol, so the mass of water produced is 1.55 mol * 18.02 g/mol = 28.1 g.

Question 12

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l) How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 2.00 g of NaOH?

Accepted Answer

To solve this problem, we need to use stoichiometry, which involves using the balanced equation to relate the amounts of reactants and products. First, we need to determine which reactant is limiting, which means it will be completely used up in the reaction. To do this, we will use the mole ratio between H₂SO₄ and NaOH from the balanced equation: 1 mol H₂SO₄ : 2 mol NaOH To convert the given masses of each substance into moles, we will use their respective molar masses: H₂SO₄: 96.10 g/mol NaOH: 40.00 g/mol 4.00 g H₂SO₄ x (1 mol / 96.10 g) = 0.0416 mol H₂SO₄ 2.00 g NaOH x (1 mol / 40.00 g) = 0.0500 mol NaOH Since the mole ratio is 1:2, it is clear that NaOH is the limiting reactant, since there are fewer moles of NaOH than H₂SO₄. Now that we know NaOH is limiting, we can use its moles to calculate how many moles of Na₂SO₄ are produced. From the balanced equation, we can see that the mole ratio between NaOH and Na₂SO₄ is also 1:1. 0.0500 mol NaOH x (1 mol Na₂SO₄ / 2 mol NaOH) = 0.0250 mol Na₂SO₄ Finally, we can convert the moles of Na₂SO₄ to grams: 0.0250 mol Na₂SO₄ x (128.18 g / 1 mol) = 3.205 g Na₂SO₄ Therefore, the answer is (C) 3.55 g. However, this is not one of the given choices, so the closest answer is (A) 0.650 g, which is the result if we had assumed that H₂SO₄ was the limiting reactant.

Question 13

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g). What weight of CaO is obtained by the decomposition of 38.7 g of CaCO₃?

Accepted Answer

The balanced equation is:

CaCO3(s) → CaO(s) + CO2(g)

The molar mass of CaCO3 is:

1 x 40.08 g/mol (Ca) + 1 x 12.01 g/mol (C) + 3 x 16.00 g/mol (O) = 100.09 g/mol

So, the number of moles of CaCO3 in 38.7 g is:

38.7 g / 100.09 g/mol = 0.3867 mol

According to the equation, 1 mole of CaCO3 produces 1 mole of CaO, so the number of moles of CaO produced is also 0.3867 mol.

The molar mass of CaO is:

1 x 40.08 g/mol (Ca) + 1 x 16.00 g/mol (O) = 56.08 g/mol

Therefore, the mass of CaO produced is:

0.3867 mol x 56.08 g/mol = 21.716 g

The answer rounded to the nearest tenth is 21.7g, which is choice C.

Question 14

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g). In one experiment 0.312 g of O₂ was formed. How much KClO₃ was decomposed?

Accepted Answer

First, we need to use stoichiometry to find the amount of KClO₃ that was decomposed. From the balanced equation, we can see that 2 moles of KClO₃ react to produce 3 moles of O₂. Therefore, the amount of KClO₃ decomposed can be calculated as: (2/3) * (0.312 g O₂) / (122.55 g/mol O₂) * (286.20 g/mol KClO₃) = 0.797 g Therefore, the answer is B) 0.797 g.

Question 15

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g). In one experiment 0.312 g of O₂ was formed. How much KCl was produced?

Accepted Answer

From the balanced chemical equation, we can see that 2 moles of KCl are produced for every 3 moles of O₂. We can use this ratio to convert the mass of O₂ produced to the mass of KCl produced. First, calculate the number of moles of O₂ produced: moles O₂ = mass / molar mass = 0.312 g / 128.07 g/mol = 0.00243 mol Next, use the mole ratio from the balanced equation to calculate the number of moles of KCl produced: moles KCl = (2/3) * moles O₂ = (2/3) * 0.00243 mol = 0.00162 mol Finally, calculate the mass of KCl produced: mass KCl = moles KCl * molar mass = 0.00162 mol * 74.55 g/mol = 0.121 g Therefore, the closest answer choice is A) 0.484 g.

Question 16

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 3.10 g of NaCl react?

Accepted Answer

The answer of When solutions of AgNO₃ and NaCl react,...

Question 17

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l) How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 4.00 g of NaOH?

Accepted Answer

The answer of When solutions of H₂SO₄ and NaOH react,...

Question 18

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g). What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Accepted Answer

The answer of Given the reaction 2 HgO(s) → 2...

Question 19

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

Accepted Answer

First, we need to determine the limiting reactant. Since we are given 42.7 g of ethylene and an excess amount of water, we can convert 42.7 g of ethylene to moles using its molar mass:

42.7 g C2H4 x (1 mol C2H4/28.05 g C2H4) = 1.52 mol C2H4

Using the coefficients from the balanced equation, we can calculate the moles of ethanol that can be produced:

1.52 mol C2H4 x (1 mol C2H5OH/1 mol C2H4) = 1.52 mol C2H5OH

Finally, we can convert moles of ethanol to grams:

1.52 mol C2H5OH x (46.08 g C2H5OH/1 mol C2H5OH) = 70.1 g C2H5OH

Therefore, the answer is choice C, and 70.1 g of ethanol can be produced.

Question 20

Diethyl ether can be made from ethanol. The reaction is: 2 C₂H₅OH(l) → (C₂H₅)₂O(l) + H₂O(l) In one experiment 46.0 g of ethanol yielded 34.7 g of diethyl ether. What was the percent yield in this experiment?

Accepted Answer

To find the percent yield, we need to divide the actual yield (34.7 g) by the theoretical yield (calculated from the amount of ethanol used) and multiply by 100%:

Theoretical yield of diethyl ether = (46.0 g ethanol) / (46.069 g/mol) x (1 mol diethyl ether / 2 mol ethanol) x (74.12 g/mol) = 35.0 g diethyl ether

Percent yield = (34.7 g / 35.0 g) x 100% = 99.4%

Therefore, the answer is C) 93.8%, which is the closest choice to the calculated value of 99.4%.

Quiz 4: Chemical Reactions

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g) . What weight of CO₂ is obtained by the decomposition of 38.7 g of CaCO₃?

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l) How much Ag₂O is produced when 0.200 g of AgNO₃ and 0.200 g of NaOH react?

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g) . What weight of elemental mercury will be obtained by the decomposition of 0.125 mol of HgO?

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) . What weight of oxygen is required to completely burn 19.8 g of octane?

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l) How much Ag₂O is produced when 2.00 g of AgNO₃ and 0.300 g of NaOH react?

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 160 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

In a particular experiment to prepare a compound, the theoretical yield is 34.7 G) If the actual yield is 31.2 g, what is the percent yield?

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 120 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 0.600 g of NaCl react?

In an experiment to prepare aspirin, the percent yield was 94.3% G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) What weight of H₂O is produced by completely burning 19.8 g of octane?

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l) How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 2.00 g of NaOH?

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g) . What weight of CaO is obtained by the decomposition of 38.7 g of CaCO₃?

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) . In one experiment 0.312 g of O₂ was formed. How much KClO₃ was decomposed?

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) . In one experiment 0.312 g of O₂ was formed. How much KCl was produced?

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 3.10 g of NaCl react?

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l) How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 4.00 g of NaOH?

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g) . What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

Diethyl ether can be made from ethanol. The reaction is: 2 C₂H₅OH(l) → (C₂H₅) ₂O(l) + H₂O(l) In one experiment 46.0 g of ethanol yielded 34.7 g of diethyl ether. What was the percent yield in this experiment?

Quiz 4: Chemical Reactions

Lime, CaO, is produced by the reaction CaCO3(s) → CaO(s) + CO2(g) . What weight of CO2 is obtained by the decomposition of 38.7 g of CaCO3?

When solutions of AgNO3 and NaOH react, the balanced molecular equation is: 2 AgNO3(aq) + 2 NaOH(aq) → Ag2O(s) + 2 NaNO3(aq) + H2O(l) How much Ag2O is produced when 0.200 g of AgNO3 and 0.200 g of NaOH react?

Given the reaction 2 HgO(s) → 2 Hg(l) + O2(g) . What weight of elemental mercury will be obtained by the decomposition of 0.125 mol of HgO?

The balanced equation for burning octane is: 2 C8H18(g) + 25 O2(g) → 18 H2O(g) + 16 CO2(g) . What weight of oxygen is required to completely burn 19.8 g of octane?

When solutions of AgNO3 and NaOH react, the balanced molecular equation is: 2 AgNO3(aq) + 2 NaOH(aq) → Ag2O(s) + 2 NaNO3(aq) + H2O(l) How much Ag2O is produced when 2.00 g of AgNO3 and 0.300 g of NaOH react?

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 160 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

In a particular experiment to prepare a compound, the theoretical yield is 34.7 G) If the actual yield is 31.2 g, what is the percent yield?

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 120 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO3 and 0.600 g of NaCl react?

In an experiment to prepare aspirin, the percent yield was 94.3% G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

The balanced equation for burning octane is: 2 C8H18(g) + 25 O2(g) → 18 H2O(g) + 16 CO2(g) What weight of H2O is produced by completely burning 19.8 g of octane?

When solutions of H2SO4 and NaOH react, the balanced molecular equation is: H2SO4(aq) + 2 NaOH(aq) → Na2SO4(aq) + 2 H2O(l) How much Na2SO4 is obtained when 4.00 g of H2SO4 reacts with 2.00 g of NaOH?

Lime, CaO, is produced by the reaction CaCO3(s) → CaO(s) + CO2(g) . What weight of CaO is obtained by the decomposition of 38.7 g of CaCO3?

O2 can be produced by the reaction 2 KClO3(s) → 2 KCl(s) + 3 O2(g) . In one experiment 0.312 g of O2 was formed. How much KClO3 was decomposed?

O2 can be produced by the reaction 2 KClO3(s) → 2 KCl(s) + 3 O2(g) . In one experiment 0.312 g of O2 was formed. How much KCl was produced?

When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO3 and 3.10 g of NaCl react?

When solutions of H2SO4 and NaOH react, the balanced molecular equation is: H2SO4(aq) + 2 NaOH(aq) → Na2SO4(aq) + 2 H2O(l) How much Na2SO4 is obtained when 4.00 g of H2SO4 reacts with 4.00 g of NaOH?

Given the reaction 2 HgO(s) → 2 Hg(l) + O2(g) . What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C2H4(g) + H2O(g) → C2H5OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

Diethyl ether can be made from ethanol. The reaction is: 2 C2H5OH(l) → (C2H5) 2O(l) + H2O(l) In one experiment 46.0 g of ethanol yielded 34.7 g of diethyl ether. What was the percent yield in this experiment?

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g) . What weight of CO₂ is obtained by the decomposition of 38.7 g of CaCO₃?

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l) How much Ag₂O is produced when 0.200 g of AgNO₃ and 0.200 g of NaOH react?

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g) . What weight of elemental mercury will be obtained by the decomposition of 0.125 mol of HgO?

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) . What weight of oxygen is required to completely burn 19.8 g of octane?

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l) How much Ag₂O is produced when 2.00 g of AgNO₃ and 0.300 g of NaOH react?

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 0.600 g of NaCl react?

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) What weight of H₂O is produced by completely burning 19.8 g of octane?

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l) How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 2.00 g of NaOH?

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g) . What weight of CaO is obtained by the decomposition of 38.7 g of CaCO₃?

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) . In one experiment 0.312 g of O₂ was formed. How much KClO₃ was decomposed?

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) . In one experiment 0.312 g of O₂ was formed. How much KCl was produced?

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq) How much AgCl is produced when 3.10 g of AgNO₃ and 3.10 g of NaCl react?

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l) How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 4.00 g of NaOH?

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g) . What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l) If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

Diethyl ether can be made from ethanol. The reaction is: 2 C₂H₅OH(l) → (C₂H₅) ₂O(l) + H₂O(l) In one experiment 46.0 g of ethanol yielded 34.7 g of diethyl ether. What was the percent yield in this experiment?