Question 1

Consider a reaction in which two reactants make one product (for example, consider the unbalanced reaction  ). You know the following: 2.0 mol A (with an excess of B) can produce a maximum of 2.0 mol C
3)0 mol B (with an excess of A) can produce a maximum of 4.0 mol C
If you react 2.0 mol A with 3.0 mol B, what is the maximum amount of C that can be produced?

Accepted Answer

The answer of Consider a reaction in which two reactants...

Question 2

Consider the equation: A + 4B  3C + 3D When equal masses of A and B are reacted, which is limiting?

Accepted Answer

The answer of Consider the equation: A + 4B ...

Question 3

Consider the following unbalanced equation:  If 1.86 g of ethanol reacts with 14.3 g of oxygen, how many moles of water are produced?

Accepted Answer

The answer of Consider the following unbalanced equation:  If...

Question 4

Consider the following reaction at 1.10 atm and 19^°C: 0.228 mol of sodium chloride, 3.03 L of ammonia, 2.00 L of carbon dioxide, and an unlimited amount of water react to form aqueous ammonium chloride and solid sodium bicarbonate. How many moles of ammonium chloride are formed in the reaction?

Accepted Answer

The answer of Consider the following reaction at 1.10 atm...

Question 5

Consider the equation:  . The molar mass of B is 50.0 g/mol. Which of the following statements is true when equal masses of A and B are reacted?

Accepted Answer

The answer of Consider the equation:  . The molar...

Question 6

Consider the following unbalanced equation: How many grams of sodium are required to completely react with 0.300 mol Na₂SiF₆?

Accepted Answer

The answer of Consider the following unbalanced equation:  How...

Question 7

Which of the following statements is always true concerning a reaction represented by the following balanced chemical equation?

Accepted Answer

The answer of Which of the following statements is always...

Question 8

For the titration of sulfuric acid (H₂SO₄) with sodium hydroxide (NaOH), how many moles of sodium hydroxide would be required to react with 1.50 L of 0.500 M sulfuric acid to reach the endpoint?

Accepted Answer

The balanced equation for the reaction is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O

From the balanced equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of sodium hydroxide. Therefore, the number of moles of sodium hydroxide required to react with the given amount of sulfuric acid can be calculated as follows:

moles of NaOH = moles of H2SO4 × 2
moles of H2SO4 = Molarity × Volume = 0.500 mol/L × 1.50 L = 0.750 mol
moles of NaOH = 0.750 mol × 2 = 1.50 mol

Therefore, the answer is C) 1.50 mol.

Question 9

When 10.0 mol of calcium metal is reacted with 3.9 mol of oxygen gas, how much calcium oxide is produced?

Accepted Answer

The balanced chemical equation for the reaction is:

2Ca + O2 → 2CaO

According to the stoichiometry of the equation, 2 moles of calcium react with 1 mole of oxygen to produce 2 moles of calcium oxide. Therefore, to determine the amount of calcium oxide produced, we need to find the limiting reactant first.

- Calcium: 10.0 mol
- Oxygen: 3.9 mol

The stoichiometric ratio of calcium to oxygen is 2:1. Therefore, if all the calcium reacts, we would need 2 × 10.0 = 20.0 mol of oxygen. Since we only have 3.9 mol of oxygen, it is the limiting reactant. This means that all the oxygen will be used up before all the calcium is consumed. We can calculate the amount of calcium oxide produced as follows:

3.9 mol O2 × (2 mol CaO/1 mol O2) = 7.8 mol CaO

Therefore, the answer is C) 7.8 mol.

Question 10

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 5.66 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of oxygen left over after the reaction is complete.

Accepted Answer

The answer of Consider that calcium metal reacts with oxygen...

Question 11

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.17 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium left over after the reaction is complete.

Accepted Answer

From the balanced chemical equation, we know that 2 mol of calcium reacts with 1 mol of oxygen gas. Therefore, the limiting reactant is oxygen gas since we only have 4.00 mol, which is not enough to react with all 6.17 mol of calcium. The balanced chemical equation also shows that for every 2 mol of calcium that reacts, 2 mol of calcium oxide is produced. Therefore, since all the oxygen gas is used up in the reaction, we will only produce 2.00 mol of calcium oxide. That leaves 6.17 mol - 2.00 mol = 4.17 mol of calcium left over unreacted.

Question 12

Consider the following unbalanced equation:  If 3.09 moles of Si were produced, how many moles of NaF were also created?

Accepted Answer

The answer of Consider the following unbalanced equation:  If...

Question 13

In the reaction between CO and Fe₃O₄, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 37.0 g Fe. Calculate the percentage yield.

Accepted Answer

Percentage yield = (actual yield/theoretical yield) x 100%
Percentage yield = (37.0 g Fe/47.2 g Fe) x 100% = 78.4%

Question 14

Equal masses of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting?

Accepted Answer

The answer of Equal masses of hydrogen gas and oxygen...

Question 15

Consider the following unbalanced equation:  If 1.70 g of ethanol reacts with 11.2 g of oxygen, how many moles of carbon dioxide are produced?

Accepted Answer

First, we need to balance the equation:

C2H5OH + 3O2 -> 2CO2 + 3H2O

Next, we convert the given masses to moles:

1.70 g C2H5OH / 46.07 g/mol C2H5OH = 0.0369 mol C2H5OH

11.2 g O2 / 32.00 g/mol O2 = 0.350 mol O2

Now, we need to determine the limiting reactant. To do this, we calculate the mole ratio of each reactant to the product:

Mole ratio for C2H5OH:

1 mol C2H5OH / 2 mol CO2

Mole ratio for O2:

3 mol O2 / 2 mol CO2

Since the mole ratio for C2H5OH is lower, it is the limiting reactant. We can use the mole ratio from the balanced equation to determine the amount of CO2 produced:

1 mol C2H5OH produces 2 mol CO2

0.0369 mol C2H5OH x (2 mol CO2 / 1 mol C2H5OH) = 0.0738 mol CO2

Therefore, the answer is C) 0.0738 mol CO2.

Question 16

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.02 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium oxide produced after the reaction is complete.

Accepted Answer

The balanced chemical equation for the reaction is 2Ca + O2 → 2CaO. According to the stoichiometry, 2 moles of Ca react with 1 mole of O2 to produce 2 moles of CaO. Since 6.02 moles of Ca would require 3.01 moles of O2 to completely react, and we have 4.00 moles of O2 available, Ca is the limiting reactant. Therefore, 6.02 moles of Ca will produce 6.02 moles of CaO.

Question 17

Ammonia reacts with oxygen to form nitrogen dioxide and water according to the following equation:  You react ammonia and oxygen, and at the end of the experiment you find that you produced 23.0 g of water and have 8.52 g of ammonia left over. Determine the mass of oxygen reacted.

Accepted Answer

First, we need to find the amount of ammonia that reacted by subtracting the amount left over from the initial amount:

Initial amount of ammonia - Amount of ammonia left over = Amount of ammonia reacted
x - 8.52 g = amount of ammonia reacted

Next, we need to use stoichiometry to find the amount of oxygen that reacted based on the amount of water produced. From the balanced equation, we can see that the ratio of ammonia to water is 4:6, which simplifies to 2:3:

2 NH3 + 3 O2 -> 2 NO + 3 H2O

So for every 3 moles of water produced, we need 2 moles of ammonia and 3 moles of oxygen.

We can use the amount of water produced to calculate the amount of oxygen needed:

23.0 g H2O x (1 mol H2O / 18.015 g H2O) x (3 mol O2 / 3 mol H2O) = 3.20 mol O2

Finally, we can use the amount of ammonia reacted and the stoichiometric ratio to find the amount of oxygen that reacted:

x - 8.52 g NH3 x (1 mol NH3 / 17.031 g NH3) x (3 mol O2 / 2 mol NH3) = 0.901 mol O2

Now that we know the amount of oxygen that reacted, we can use its molar mass to calculate its mass:

0.901 mol O2 x 31.998 g/mol O2 = 28.9 g O2

Therefore, the correct answer is E) 47.7 g of oxygen.

Question 18

You react 25.0 g hydrogen gas with 73.7 g oxygen gas. Determine the mass of water that can be produced from these reactants.

Accepted Answer

The balanced chemical equation for the reaction is 2H₂ + O₂ → 2H₂O. The molar mass of H₂ is 2 g/mol, and O₂ is 32 g/mol. 25.0 g H₂ is 12.5 mol, and 73.7 g O₂ is 2.3 mol. O₂ is the limiting reactant, producing 2.3 mol of H₂O, which is 41.4 g. However, the mass of water produced is calculated based on the limiting reactant, which is oxygen, and the total mass of reactants is 98.7 g, so the mass of water produced is 83.0 g.

Question 19

Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 4.52 mol of magnesium and 4.52 mol of hydrochloric acid are reacted, how many moles of hydrogen gas are produced?

Accepted Answer

The balanced chemical equation for this reaction is:
Mg + 2HCl → MgCl2 + H2
According to the balanced equation, one mole of magnesium reacts with two moles of hydrochloric acid to produce one mole of hydrogen gas. Therefore, if 4.52 mol of magnesium and 4.52 mol of hydrochloric acid are reacted, the limiting reactant is magnesium, and 2.26 mol of hydrogen gas are produced.

Question 20

Reacting 3.00 mol nitrogen gas with 3.50 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation?

Accepted Answer

The answer of Reacting 3.00 mol nitrogen gas with 3.50...

Quiz 9: Chemical Quantities

Consider the equation: A + 4B 3C + 3D When equal masses of A and B are reacted, which is limiting?

Consider the following unbalanced equation: If 1.86 g of ethanol reacts with 14.3 g of oxygen, how many moles of water are produced?

Consider the following reaction at 1.10 atm and 19^°C: 0.228 mol of sodium chloride, 3.03 L of ammonia, 2.00 L of carbon dioxide, and an unlimited amount of water react to form aqueous ammonium chloride and solid sodium bicarbonate. How many moles of ammonium chloride are formed in the reaction?

Consider the equation: . The molar mass of B is 50.0 g/mol. Which of the following statements is true when equal masses of A and B are reacted?

Consider the following unbalanced equation: How many grams of sodium are required to completely react with 0.300 mol Na₂SiF₆?

Which of the following statements is always true concerning a reaction represented by the following balanced chemical equation?

For the titration of sulfuric acid (H₂SO₄) with sodium hydroxide (NaOH) , how many moles of sodium hydroxide would be required to react with 1.50 L of 0.500 M sulfuric acid to reach the endpoint?

When 10.0 mol of calcium metal is reacted with 3.9 mol of oxygen gas, how much calcium oxide is produced?

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 5.66 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of oxygen left over after the reaction is complete.

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.17 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium left over after the reaction is complete.

Consider the following unbalanced equation: If 3.09 moles of Si were produced, how many moles of NaF were also created?

In the reaction between CO and Fe₃O₄, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 37.0 g Fe. Calculate the percentage yield.

Equal masses of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting?

Consider the following unbalanced equation: If 1.70 g of ethanol reacts with 11.2 g of oxygen, how many moles of carbon dioxide are produced?

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.02 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium oxide produced after the reaction is complete.

Ammonia reacts with oxygen to form nitrogen dioxide and water according to the following equation: You react ammonia and oxygen, and at the end of the experiment you find that you produced 23.0 g of water and have 8.52 g of ammonia left over. Determine the mass of oxygen reacted.

You react 25.0 g hydrogen gas with 73.7 g oxygen gas. Determine the mass of water that can be produced from these reactants.

Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 4.52 mol of magnesium and 4.52 mol of hydrochloric acid are reacted, how many moles of hydrogen gas are produced?

Reacting 3.00 mol nitrogen gas with 3.50 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation?

Quiz 9: Chemical Quantities

Consider the equation: A + 4B 3C + 3D When equal masses of A and B are reacted, which is limiting?

Consider the following unbalanced equation: If 1.86 g of ethanol reacts with 14.3 g of oxygen, how many moles of water are produced?

Consider the following reaction at 1.10 atm and 19°C: 0.228 mol of sodium chloride, 3.03 L of ammonia, 2.00 L of carbon dioxide, and an unlimited amount of water react to form aqueous ammonium chloride and solid sodium bicarbonate. How many moles of ammonium chloride are formed in the reaction?

Consider the equation: . The molar mass of B is 50.0 g/mol. Which of the following statements is true when equal masses of A and B are reacted?

Consider the following unbalanced equation: How many grams of sodium are required to completely react with 0.300 mol Na2SiF6?

Which of the following statements is always true concerning a reaction represented by the following balanced chemical equation?

For the titration of sulfuric acid (H2SO4) with sodium hydroxide (NaOH) , how many moles of sodium hydroxide would be required to react with 1.50 L of 0.500 M sulfuric acid to reach the endpoint?

When 10.0 mol of calcium metal is reacted with 3.9 mol of oxygen gas, how much calcium oxide is produced?

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 5.66 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of oxygen left over after the reaction is complete.

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.17 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium left over after the reaction is complete.

Consider the following unbalanced equation: If 3.09 moles of Si were produced, how many moles of NaF were also created?

In the reaction between CO and Fe3O4, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 37.0 g Fe. Calculate the percentage yield.

Equal masses of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting?

Consider the following unbalanced equation: If 1.70 g of ethanol reacts with 11.2 g of oxygen, how many moles of carbon dioxide are produced?

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.02 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium oxide produced after the reaction is complete.

Ammonia reacts with oxygen to form nitrogen dioxide and water according to the following equation: You react ammonia and oxygen, and at the end of the experiment you find that you produced 23.0 g of water and have 8.52 g of ammonia left over. Determine the mass of oxygen reacted.

You react 25.0 g hydrogen gas with 73.7 g oxygen gas. Determine the mass of water that can be produced from these reactants.

Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 4.52 mol of magnesium and 4.52 mol of hydrochloric acid are reacted, how many moles of hydrogen gas are produced?

Reacting 3.00 mol nitrogen gas with 3.50 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation?

Consider the following reaction at 1.10 atm and 19^°C: 0.228 mol of sodium chloride, 3.03 L of ammonia, 2.00 L of carbon dioxide, and an unlimited amount of water react to form aqueous ammonium chloride and solid sodium bicarbonate. How many moles of ammonium chloride are formed in the reaction?

Consider the following unbalanced equation: How many grams of sodium are required to completely react with 0.300 mol Na₂SiF₆?

For the titration of sulfuric acid (H₂SO₄) with sodium hydroxide (NaOH) , how many moles of sodium hydroxide would be required to react with 1.50 L of 0.500 M sulfuric acid to reach the endpoint?

In the reaction between CO and Fe₃O₄, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 37.0 g Fe. Calculate the percentage yield.