Question 1

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and excess chlorine?

Accepted Answer

The equation provided is not balanced and does not relate to aluminum chloride. Assuming a balanced equation for aluminum and chlorine to form aluminum chloride (2Al + 3Cl2 → 2AlCl3), 4.5 moles of aluminum would produce 4.5 moles of aluminum chloride when chlorine is in excess.

Question 2

Use the balanced equation HS1U1B12S1U1B0SOS1U1B14S1U1B0 + Cu → SOS1U1B12S1U1B0 + HS1U1B12S1U1B0O + CuSOS1U1B14S1U1B0 to answer the following question(s).
-The theoretical number of moles of copper that will react with 4 moles of sulfuric acid is ________.

Accepted Answer

The balanced equation shows that 1 mole of copper reacts with 2 moles of sulfuric acid. Therefore, 4 moles of sulfuric acid will react with 2 moles of copper.

Question 3

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-0.011 moles of an element has a mass of 2.56 g. This element is ________.

Accepted Answer

The answer of Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 →...

Question 4

For the process 2H₂ + O₂ → 2H₂O, which reactant is the limiting reagent if 6 mol of H₂ and 4 mol of O₂ are used?

Accepted Answer

The balanced equation shows that 2 moles of H₂ react with 1 mole of O₂. With 6 moles of H₂, you need 3 moles of O₂. Since you have 4 moles of O₂, H₂ is the limiting reagent.

Question 5

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-What is the % yield if 52 g ammonia produce 45 g NO?

Accepted Answer

The answer of Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 →...

Question 6

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-How many grams of ammonia are consumed if 45 g NO are formed in a 100% yield?

Accepted Answer

The answer of Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 →...

Question 7

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s). -The maximum amount of IF₇ that can be obtained from 25.0 g fluorine in the equation I₂ + F₂ → IF₇ is ________.

Accepted Answer

First, we need to balance the equation given in the question. The balanced equation is: 2I₂ + 5F₂ → 2IF₇ Next, we need to find the limiting reactant. We have 25.0 g of fluorine, so we need to convert it to moles: 25.0 g F2 / (2 x 18.9984 g/mol) = 0.658 mol F2 Now we can use stoichiometry to find the theoretical yield of IF₇: 0.658 mol F2 x (2 mol IF₇ / 5 mol F2) x (253.808 g/mol) = 48.9 g IF₇ Therefore, the maximum amount of IF₇ that can be obtained is 48.9 g. Choice B is the correct answer.

Question 8

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s). -In the equation N₂ + 2 O₂ → 2 NO₂, 14 g of nitrogen will yield ________ g nitrogen dioxide.

Accepted Answer

The equation given in the question is not directly relevant to the problem, so it can be ignored. Instead, we can use the stoichiometry of the balanced equation given in the problem to determine the amount of nitrogen dioxide produced from 14 g of nitrogen:

1 mol of nitrogen = 28.0 g
1 mol of nitrogen dioxide = 46.0 g

So, using the given equation, we can set up a proportion:

14 g of nitrogen / 28.0 g/mol = x g of nitrogen dioxide / 46.0 g/mol

Solving for x, we get:

x = (14 g) * (46.0 g/mol) / (28.0 g/mol) = 23 g

Therefore, the answer is B) 46.

Question 9

In the above compound 0.842 g chlorine will combine with ________ g of sulfur to produce the same compound.

Accepted Answer

The compound is likely to be sulfur dichloride (SCl2), where the molar ratio of sulfur to chlorine is 1:2. The molar mass of chlorine is approximately 35.5 g/mol, and sulfur is approximately 32.1 g/mol. For 0.842 g of chlorine, the mass of sulfur needed is calculated using the ratio of their molar masses, resulting in approximately 0.379 g of sulfur.

Question 10

Use the balanced equation HS1U1B12S1U1B0SOS1U1B14S1U1B0 + Cu → SOS1U1B12S1U1B0 + HS1U1B12S1U1B0O + CuSOS1U1B14S1U1B0 to answer the following question(s).
-The % yield of an experiment in which two moles copper was used and 18 g water was isolated is ________.

Accepted Answer

The answer of Use the balanced equation HS1U1B12S1U1B0SOS1U1B14S1U1B0 + Cu...

Question 11

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-If 14 kg of nitrogen yields 23 kg nitrogen dioxide, the % yield for the reaction is ________.

Accepted Answer

The balanced equation shows that 1 mol of nitrogen reacts with 1 mol of oxygen to produce 2 mol of nitrogen dioxide. Therefore, the theoretical yield of nitrogen dioxide from 14 kg of nitrogen would be:

(23 kg N2O4 / 2 mol N2O4) x (1 mol N2 / 1 mol N2O4) x (28 g N2 / 1 mol N2) = 13840 g N2 => 13.84 kg N2

The actual yield is not given, but assuming it is 13.84 kg, the percent yield would be:

(13.84 kg / 14 kg) x 100% = 98.86% ≈ 50% (rounded to the nearest whole number)

Therefore, the best choice is B.

Question 12

0.68 g of sulfur combine with 1.51 g of chlorine. The empirical formula of this compound is ________.

Accepted Answer

To find the empirical formula, calculate the moles of each element: Moles of S = 0.68 g / 32.07 g/mol = 0.0212 mol; Moles of Cl = 1.51 g / 35.45 g/mol = 0.0426 mol. The ratio of S to Cl is approximately 1:2, so the empirical formula is SCl₂.

Question 13

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-If 4 moles nitrogen produces 2 moles nitrogen dioxide, the % yield is ________.

Accepted Answer

The answer of Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 →...

Question 14

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s). -In the equation N₂ + 2 O₂ → 2 NO₂, 14 g of nitrogen will react with ________ g oxygen.

Accepted Answer

By comparing the coefficients in the two equations, we can see that one mole of nitrogen reacts with two moles of oxygen to produce two moles of NO₂. Using the molar mass of nitrogen (14 g/mol), we can calculate the amount of oxygen needed: 1 mol N + 2 mol O → 2 mol NO₂ 14 g N + ? g O → 92 g NO₂ ? g O = (92 g NO₂/2 mol NO₂) × (2 mol O/1 mol N) × (32 g O/mol O) ? g O = 64 g O

Question 15

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-The number of moles of chlorine, (Cl atoms)in 12.5 g carbon tetrachloride is ________.

Accepted Answer

The given chemical equation is not relevant to finding the number of moles of chlorine in carbon tetrachloride. However, we can use the molar mass of carbon tetrachloride (CCl4) to find the number of moles of carbon tetrachloride in 12.5 g. 
Molar mass of CCl4 = (12.01 + 4 x 35.45) g/mol = 153.82 g/mol 
Number of moles of CCl4 = 12.5 g / 153.82 g/mol = 0.0813 mol 
Each molecule of carbon tetrachloride contains 4 chlorine atoms. 
Number of moles of chlorine atoms = 4 x 0.0813 mol = 0.3252 mol 
Therefore, the number of moles of chlorine atoms in 12.5 g carbon tetrachloride is 0.325, which is closest to option C (0.325).

Question 16

Use the balanced equation HS1U1B12S1U1B0SOS1U1B14S1U1B0 + Cu → SOS1U1B12S1U1B0 + HS1U1B12S1U1B0O + CuSOS1U1B14S1U1B0 to answer the following question(s).
-The theoretical number of moles of water produced from 4 moles of sulfuric acid is ________.

Accepted Answer

The balanced equation shows that 1 mole of sulfuric acid (HS1U1B12S1U1B0SOS1U1B14S1U1B0) produces 1 mole of water (HS1U1B12S1U1B0O). Therefore, 4 moles of sulfuric acid will produce 4 moles of water.

Question 17

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-The balanced equation involves the corresponding coefficients ________.

Accepted Answer

The answer of Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 →...

Question 18

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-What is the mass of NO expected if 104 g of ammonia are consumed in a 100% yield?

Accepted Answer

From the equation, we can see that the ratio of NH3 to NO is 1:1. Therefore, if 104 g of NH3 is consumed in a 100% yield, the mass of NO produced will also be 104 g. However, we must convert the formula weight of NH3 (17 g/mol) to the formula weight of NO (30 g/mol) to determine the mass of NO produced.

104 g NH3 x (1 mol NH3/17 g NH3) x (1 mol NO/1 mol NH3) x (30 g NO/1 mol NO) = 180 g NO

Therefore, the mass of NO expected is 180 g. Choice C is correct.

Question 19

Use the balanced equation HS1U1B12S1U1B0SOS1U1B14S1U1B0 + Cu → SOS1U1B12S1U1B0 + HS1U1B12S1U1B0O + CuSOS1U1B14S1U1B0 to answer the following question(s).
-The theoretical mass of sulfur dioxide produced from two moles of sulfuric acid is ________.

Accepted Answer

The answer of Use the balanced equation HS1U1B12S1U1B0SOS1U1B14S1U1B0 + Cu...

Question 20

Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 → NO + HS1U1B12S1U1B0O to answer the following question(s).
-How many grams of oxygen will react with 20 g of ammonia?

Accepted Answer

The answer of Use the equation NHS1U1B13S1U1B0 + OS1U1B12S1U1B0 →...

Quiz 9: Stoichiometry and the Mole

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and excess chlorine?

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The theoretical number of moles of copper that will react with 4 moles of sulfuric acid is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -0.011 moles of an element has a mass of 2.56 g. This element is ________.

For the process 2H₂ + O₂ → 2H₂O, which reactant is the limiting reagent if 6 mol of H₂ and 4 mol of O₂ are used?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -What is the % yield if 52 g ammonia produce 45 g NO?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -How many grams of ammonia are consumed if 45 g NO are formed in a 100% yield?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -The maximum amount of IF₇ that can be obtained from 25.0 g fluorine in the equation I₂ + F₂ → IF₇ is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -In the equation N₂ + 2 O₂ → 2 NO₂, 14 g of nitrogen will yield ________ g nitrogen dioxide.

In the above compound 0.842 g chlorine will combine with ________ g of sulfur to produce the same compound.

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The % yield of an experiment in which two moles copper was used and 18 g water was isolated is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -If 14 kg of nitrogen yields 23 kg nitrogen dioxide, the % yield for the reaction is ________.

0.68 g of sulfur combine with 1.51 g of chlorine. The empirical formula of this compound is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -If 4 moles nitrogen produces 2 moles nitrogen dioxide, the % yield is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -In the equation N₂ + 2 O₂ → 2 NO₂, 14 g of nitrogen will react with ________ g oxygen.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -The number of moles of chlorine, (Cl atoms) in 12.5 g carbon tetrachloride is ________.

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The theoretical number of moles of water produced from 4 moles of sulfuric acid is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -The balanced equation involves the corresponding coefficients ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -What is the mass of NO expected if 104 g of ammonia are consumed in a 100% yield?

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The theoretical mass of sulfur dioxide produced from two moles of sulfuric acid is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -How many grams of oxygen will react with 20 g of ammonia?

Quiz 9: Stoichiometry and the Mole

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and excess chlorine?

Use the balanced equation H2SO4 + Cu → SO2 + H2O + CuSO4 to answer the following question(s) . -The theoretical number of moles of copper that will react with 4 moles of sulfuric acid is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -0.011 moles of an element has a mass of 2.56 g. This element is ________.

For the process 2H2 + O2 → 2H2O, which reactant is the limiting reagent if 6 mol of H2 and 4 mol of O2 are used?

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -What is the % yield if 52 g ammonia produce 45 g NO?

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -How many grams of ammonia are consumed if 45 g NO are formed in a 100% yield?

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -The maximum amount of IF7 that can be obtained from 25.0 g fluorine in the equation I2 + F2 → IF7 is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -In the equation N2 + 2 O2 → 2 NO2, 14 g of nitrogen will yield ________ g nitrogen dioxide.

In the above compound 0.842 g chlorine will combine with ________ g of sulfur to produce the same compound.

Use the balanced equation H2SO4 + Cu → SO2 + H2O + CuSO4 to answer the following question(s) . -The % yield of an experiment in which two moles copper was used and 18 g water was isolated is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -If 14 kg of nitrogen yields 23 kg nitrogen dioxide, the % yield for the reaction is ________.

0.68 g of sulfur combine with 1.51 g of chlorine. The empirical formula of this compound is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -If 4 moles nitrogen produces 2 moles nitrogen dioxide, the % yield is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -In the equation N2 + 2 O2 → 2 NO2, 14 g of nitrogen will react with ________ g oxygen.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -The number of moles of chlorine, (Cl atoms) in 12.5 g carbon tetrachloride is ________.

Use the balanced equation H2SO4 + Cu → SO2 + H2O + CuSO4 to answer the following question(s) . -The theoretical number of moles of water produced from 4 moles of sulfuric acid is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -The balanced equation involves the corresponding coefficients ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -What is the mass of NO expected if 104 g of ammonia are consumed in a 100% yield?

Use the balanced equation H2SO4 + Cu → SO2 + H2O + CuSO4 to answer the following question(s) . -The theoretical mass of sulfur dioxide produced from two moles of sulfuric acid is ________.

Use the equation NH3 + O2 → NO + H2O to answer the following question(s) . -How many grams of oxygen will react with 20 g of ammonia?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and excess chlorine?

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The theoretical number of moles of copper that will react with 4 moles of sulfuric acid is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -0.011 moles of an element has a mass of 2.56 g. This element is ________.

For the process 2H₂ + O₂ → 2H₂O, which reactant is the limiting reagent if 6 mol of H₂ and 4 mol of O₂ are used?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -What is the % yield if 52 g ammonia produce 45 g NO?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -How many grams of ammonia are consumed if 45 g NO are formed in a 100% yield?

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -The maximum amount of IF₇ that can be obtained from 25.0 g fluorine in the equation I₂ + F₂ → IF₇ is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -In the equation N₂ + 2 O₂ → 2 NO₂, 14 g of nitrogen will yield ________ g nitrogen dioxide.

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The % yield of an experiment in which two moles copper was used and 18 g water was isolated is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -If 14 kg of nitrogen yields 23 kg nitrogen dioxide, the % yield for the reaction is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -If 4 moles nitrogen produces 2 moles nitrogen dioxide, the % yield is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -In the equation N₂ + 2 O₂ → 2 NO₂, 14 g of nitrogen will react with ________ g oxygen.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -The number of moles of chlorine, (Cl atoms) in 12.5 g carbon tetrachloride is ________.

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The theoretical number of moles of water produced from 4 moles of sulfuric acid is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -The balanced equation involves the corresponding coefficients ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -What is the mass of NO expected if 104 g of ammonia are consumed in a 100% yield?

Use the balanced equation H₂SO₄ + Cu → SO₂ + H₂O + CuSO₄ to answer the following question(s) . -The theoretical mass of sulfur dioxide produced from two moles of sulfuric acid is ________.

Use the equation NH₃ + O₂ → NO + H₂O to answer the following question(s) . -How many grams of oxygen will react with 20 g of ammonia?