Question 1

Give the empirical formula for each of the following compounds: H₂O, H₂O₂, NH₃, N₂H₄, C₁₂H₂₂O₁₁, Al₂Cl₆.

Accepted Answer

The answer of Give the empirical formula for each of...

Question 2

Eugenol, a component of clove oil, is 73.15% C, 7.36% H, and 19.49% O; its molar mass is 164.19 g/mol.What is its molecular formula?

Accepted Answer

The answer of Eugenol, a component of clove oil, is...

Question 3

White phosphorus (123.88 g/mol) is produced by the reaction of calcium phosphate (310.18 g/mol), silicon dioxide (60.09 g/mol), and carbon (12.01 g/mol).How many grams of CO (28.01 g/mol) are produced as a by-product when 1.500*103 g SiO₂ reacts with excess (Ca₃PO₄)₂ and C? Assume 100% yield. 2 Ca₃ (PO₄ )₂ (s) + 6 Si O₂ (s) + 10 Cs) $\rightarrow$ P4 (s) + 6 CaSi O₃ (s) + 10 CO(g)

Accepted Answer

The answer of White phosphorus (123.88 g/mol) is produced by...

Question 4

Some indoor air purification systems work by converting some of the oxygen in the air to ozone, which oxidizes mold, mildew spores, and other biological pollutants.One such system supposedly generates 5.0 g O₃ per hour by passing dry air through the purifier at a rate of 5.0 L/min.If 1.0 L of air contains 0.28 g of oxygen, what percent of the O₂ molecules are converted to O₃ molecules?

Accepted Answer

The answer of Some indoor air purification systems work by...

Question 5

Elemental phosphorus (123.88 g/mol) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.What is the theoretical yield in grams) of PF ₃ (87.97 g/mol) when 15.0 g P₄ reacts with 25.0 g F₂ (38.00 g/mol)? P₄(s) +6 F₂ (g) $\rightarrow$ 4 PF₃ (g)

Accepted Answer

The answer of Elemental phosphorus (123.88 g/mol) reacts vigorously with...

Question 6

Acetylsalicylic acid, the active ingredient in aspirin, contains carbon, hydrogen, and oxygen.The complete combustion of 1.000 g acetylsalicylic acid produces 2.199 g CO₂ and 0.400 g H₂O.Mass spectrometry experiments showed that its molar mass is less than 200 g/mol.What is the molecular formula of acetylsalicylic acid?

Accepted Answer

The answer of Acetylsalicylic acid, the active ingredient in aspirin,...

Question 7

Mesitylene is a liquid hydrocarbon.If 0.115 g of this compound is burned in pure oxygen to give 0.3790 g CO₂ and 0.1035 g H₂O, what is the empirical formula of the compound?

Accepted Answer

The answer of Mesitylene is a liquid hydrocarbon.If 0.115 g...

Question 8

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Accepted Answer

The answer of Nitric oxide (30.01 g/mol) can be produced...

Question 9

Elemental phosphorus (P₄) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.How many grams of PF₃ (87.97 g/mol) can be produced using excess fluorine (38.00 g/mol) and 5.49 g P₄ (123.88 g/mol)? P ₄ (s) + 6 F₂ (g) $\rightarrow$4 PF₃ (g)

Accepted Answer

The answer of Elemental phosphorus (P₄) reacts vigorously with halogens...

Question 10

Cyanidin, a pigment found in many red berries, such as grapes, raspberries, and cranberries, contains carbon, hydrogen, and oxygen.The complete combustion of a 2.0000 g sample in excess O₂ produces 4.5964 g CO₂ and 0.6901 g H₂O.Mass spectrometry experiments showed that cyanidin's molecular mass is approximately 290 amu.What is the molecular formula of cyanidin?

Accepted Answer

The answer of Cyanidin, a pigment found in many red...

Question 11

List three reasons why the actual yield for a chemical reaction may differ from the theoretical yield.

Accepted Answer

The answer of List three reasons why the actual yield...

Question 12

During fermentation, yeast converts glucose (180.2 g/mol) into ethanol (46.08 g/mol) and carbon dioxide (44.01 g/mol).The unbalanced reaction equation is given below.Balance the equation and find the percent yield for the reaction if 150.0 g of glucose yields 75.0 mL of ethanol (d =0.789 g/mL). C₆ H₁₂ O₆ (aq) $\rightarrow$ C₂ H₅ OH(aq) + CO₂ (g)

Accepted Answer

The answer of During fermentation, yeast converts glucose (180.2 g/mol)...

Question 13

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 *10² g CO and 8.00 * 10² g Fe₂O₃ were allowed to react? Fe₂O₃ (s) + 3 CO(g) $\rightarrow$ 2 Fe(s) + 3 CO₂ (g)

Accepted Answer

The answer of Carbon monoxide (28.01 g/mol) is used in...

Question 14

Acrylonitrile (C₃H₃N, 53.07 g/mol) can be produced from propylene (C₃H₆, 42.09 g/mol) according to the reaction shown below.In a particular experiment, 125 g C₃H₆ reacts with 175 g NO (30.01 g/mol) and 105 g C₃H₃N is produced.What is the percent yield for the reaction? 4 C₃ H₆ (g) + 6 NO(g) $\rightarrow$ 4 C₃ H₃ N(l) +6 H₂ O(l) + N₂ (g)

Accepted Answer

The answer of Acrylonitrile (C₃H₃N, 53.07 g/mol) can be produced...

Question 15

TiCl₄ (189.68 g/mol), a source of Ti metal, can be produced from titanium dioxide (79.87 g/mol), carbon (12.01 g/mol), and chlorine gas (70.90 g/mol).Identify the limiting reactant if 195 g TiO₂ and 325 g Cl₂ react in the presence of excess C.Assuming 100% yield, calculate the mass of TiCl ₄ produced. 3 Ti O₂ (s) + 4 C(s) + 6 CL₂ (g) $\rightarrow$ 3 Ti CL₄ (s) + 2 CO₂ (g) + 2 CO(g)

Accepted Answer

The answer of TiCl₄ (189.68 g/mol), a source of Ti...

Question 16

Diethyl azodicarboxylate, or DEAD, is an explosive compound with the empirical formula C₃H₅NO₂ and a molecular mass of approximately 174 amu.Find its molecular formula.

Accepted Answer

The answer of Diethyl azodicarboxylate, or DEAD, is an explosive...

Question 17

Which of the following oxides of nitrogen have the same empirical formulas? N₂O, NO, NO₂, N₂O₂, N₂O₄

Accepted Answer

The answer of Which of the following oxides of nitrogen...

Question 18

Acrylonitrile (53.07 g/mol) can be produced from propylene (42.09 g/mol) according to the reaction shown below.Find the percent yield if 1250 g C₃H₆ produces 722 g H₂O (18.02 g/mol) as a by-product. 4 C₃ H₆ (g) + 6 NO(g) $\rightarrow$ 4 C₃ H₃ N(l) +6 H₂O(l) + N₂ (g)

Accepted Answer

The answer of Acrylonitrile (53.07 g/mol) can be produced from...

Question 19

Traumatic acid, an organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen.Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H.What is its molecular formula?

Accepted Answer

The answer of Traumatic acid, an organic acid with a...

Question 20

A burner in a gas grill mixes 20 volumes of air for every one volume of propane (C₃H₈).Is the mixture produced by this burner rich (excess propane), lean (excess oxygen), or just right (a stoichiometric mixture of propane and oxygen)? Assume that the volume of gas is directly proportional to the number of moles of gas and that air is 21% oxygen by volume.

Accepted Answer

The answer of A burner in a gas grill mixes...

Quiz 7: Stoichiometry Mass Relationships and Chemical Reactions

Give the empirical formula for each of the following compounds: H₂O, H₂O₂, NH₃, N₂H₄, C₁₂H₂₂O₁₁, Al₂Cl₆.

Eugenol, a component of clove oil, is 73.15% C, 7.36% H, and 19.49% O; its molar mass is 164.19 g/mol.What is its molecular formula?

Elemental phosphorus (123.88 g/mol) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.What is the theoretical yield in grams) of PF ₃ (87.97 g/mol) when 15.0 g P₄ reacts with 25.0 g F₂ (38.00 g/mol)? P₄(s) +6 F₂ (g) $\rightarrow$ 4 PF₃ (g)

Mesitylene is a liquid hydrocarbon.If 0.115 g of this compound is burned in pure oxygen to give 0.3790 g CO₂ and 0.1035 g H₂O, what is the empirical formula of the compound?

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Elemental phosphorus (P₄) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.How many grams of PF₃ (87.97 g/mol) can be produced using excess fluorine (38.00 g/mol) and 5.49 g P₄ (123.88 g/mol)? P ₄ (s) + 6 F₂ (g) $\rightarrow$ 4 PF₃ (g)

List three reasons why the actual yield for a chemical reaction may differ from the theoretical yield.

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 10² g CO and 8.00 10² g Fe₂O₃ were allowed to react? Fe₂O₃ (s) + 3 CO(g) $\rightarrow$ 2 Fe(s) + 3 CO₂ (g)

Diethyl azodicarboxylate, or DEAD, is an explosive compound with the empirical formula C₃H₅NO₂ and a molecular mass of approximately 174 amu.Find its molecular formula.

Which of the following oxides of nitrogen have the same empirical formulas? N₂O, NO, NO₂, N₂O₂, N₂O₄

Acrylonitrile (53.07 g/mol) can be produced from propylene (42.09 g/mol) according to the reaction shown below.Find the percent yield if 1250 g C₃H₆ produces 722 g H₂O (18.02 g/mol) as a by-product. 4 C₃ H₆ (g) + 6 NO(g) $\rightarrow$ 4 C₃ H₃ N(l) +6 H₂O(l) + N₂ (g)

Traumatic acid, an organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen.Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H.What is its molecular formula?

Quiz 7: Stoichiometry Mass Relationships and Chemical Reactions

Give the empirical formula for each of the following compounds: H2O, H2O2, NH3, N2H4, C12H22O11, Al2Cl6.

Eugenol, a component of clove oil, is 73.15% C, 7.36% H, and 19.49% O; its molar mass is 164.19 g/mol.What is its molecular formula?

Elemental phosphorus (123.88 g/mol) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.What is the theoretical yield in grams) of PF 3 (87.97 g/mol) when 15.0 g P4 reacts with 25.0 g F2 (38.00 g/mol)? P4 (s) +6 F2 (g) →\rightarrow→ 4 PF3 (g)

Mesitylene is a liquid hydrocarbon.If 0.115 g of this compound is burned in pure oxygen to give 0.3790 g CO2 and 0.1035 g H2O, what is the empirical formula of the compound?

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH3 and 150 g O2 react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH3 (g) + 5O2 (g) →\rightarrow→ 4 NO(g) +6H2 O(l)

Elemental phosphorus (P4) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.How many grams of PF3 (87.97 g/mol) can be produced using excess fluorine (38.00 g/mol) and 5.49 g P4 (123.88 g/mol)? P 4 (s) + 6 F2 (g) →\rightarrow→ 4 PF3 (g)

List three reasons why the actual yield for a chemical reaction may differ from the theoretical yield.

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 *102 g CO and 8.00 * 102 g Fe2O3 were allowed to react? Fe 2 O3 (s) + 3 CO(g) →\rightarrow→ 2 Fe(s) + 3 CO2 (g)

Diethyl azodicarboxylate, or DEAD, is an explosive compound with the empirical formula C3H5NO2 and a molecular mass of approximately 174 amu.Find its molecular formula.

Which of the following oxides of nitrogen have the same empirical formulas? N2O, NO, NO2, N2O2, N2O4

Acrylonitrile (53.07 g/mol) can be produced from propylene (42.09 g/mol) according to the reaction shown below.Find the percent yield if 1250 g C3H6 produces 722 g H2O (18.02 g/mol) as a by-product. 4 C3 H6 (g) + 6 NO(g) →\rightarrow→ 4 C3 H3 N(l) +6 H2O(l) + N2 (g)

Traumatic acid, an organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen.Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H.What is its molecular formula?

Give the empirical formula for each of the following compounds: H₂O, H₂O₂, NH₃, N₂H₄, C₁₂H₂₂O₁₁, Al₂Cl₆.

Elemental phosphorus (123.88 g/mol) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.What is the theoretical yield in grams) of PF ₃ (87.97 g/mol) when 15.0 g P₄ reacts with 25.0 g F₂ (38.00 g/mol)? P₄(s) +6 F₂ (g) $\rightarrow$ 4 PF₃ (g)

Mesitylene is a liquid hydrocarbon.If 0.115 g of this compound is burned in pure oxygen to give 0.3790 g CO₂ and 0.1035 g H₂O, what is the empirical formula of the compound?

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Elemental phosphorus (P₄) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.How many grams of PF₃ (87.97 g/mol) can be produced using excess fluorine (38.00 g/mol) and 5.49 g P₄ (123.88 g/mol)? P ₄ (s) + 6 F₂ (g) $\rightarrow$ 4 PF₃ (g)

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 10² g CO and 8.00 10² g Fe₂O₃ were allowed to react? Fe₂O₃ (s) + 3 CO(g) $\rightarrow$ 2 Fe(s) + 3 CO₂ (g)

Diethyl azodicarboxylate, or DEAD, is an explosive compound with the empirical formula C₃H₅NO₂ and a molecular mass of approximately 174 amu.Find its molecular formula.

Which of the following oxides of nitrogen have the same empirical formulas? N₂O, NO, NO₂, N₂O₂, N₂O₄

Acrylonitrile (53.07 g/mol) can be produced from propylene (42.09 g/mol) according to the reaction shown below.Find the percent yield if 1250 g C₃H₆ produces 722 g H₂O (18.02 g/mol) as a by-product. 4 C₃ H₆ (g) + 6 NO(g) $\rightarrow$ 4 C₃ H₃ N(l) +6 H₂O(l) + N₂ (g)