Question 1

A compound used in a polymer research project contains carbon, hydrogen, and nitrogen. The composition of the compound is: carbon, 58.774%; hydrogen, 13.810%; nitrogen, 27.416%. Determine the empirical formula of the compound. Hint: Assume you have 100 grams of this substance and use moles to relate the mass of one element to another.

Accepted Answer

The answer of A compound used in a polymer research...

Question 2

A compound contains potassium, sulfur, and oxygen. The composition of the compound is: potassium, 49.410%; sulfur, 20.261%. Determine the empirical formula of the compound. Hint: Assume you have 100 grams of this substance and use moles to relate the mass of one element to another.

Accepted Answer

The answer of A compound contains potassium, sulfur, and oxygen....

Question 3

A new compound contains nitrogen, hydrogen, boron, and fluorine. The composition of the compound is: nitrogen, 13.360%; hydrogen, 3.8455%; boron, 10.312%. Determine the empirical formula of the compound. Hint: Assume you have 100 grams of this substance and use moles to relate the mass of one element to another.

Accepted Answer

The empirical formula of the compound is NH4BF4. This can be determined by assuming that you have 100 grams of the compound and using moles to relate the mass of one element to another. The molar mass of the compound is 103.83 g/mol. The empirical formula is the simplest whole number ratio of the elements in the compound. In this case, the empirical formula is NH4BF4.

Question 4

A freshly prepared compound contains potassium, hydrogen, phosphorus, and oxygen. The composition of the compound is: potassium, 44.895%; hydrogen, 0.5787%; phosphorus, 17.783%. Determine the empirical formula of the compound. Hint: Assume you have 100 grams of this substance and use moles to relate the mass of one element to another.

Accepted Answer

The empirical formula of the compound is K2HPO4. This can be determined by assuming you have 100 grams of this substance and using moles to relate the mass of one element to another. The molar mass of the compound is 136.09 g/mol. The empirical formula is the simplest whole number ratio of the elements in the compound. In this case, the empirical formula is K2HPO4.

Question 5

A 4.626 g sample of a hydrocarbon, upon combustion analysis, yielded 6.484 grams of carbon dioxide. What is the percent, by mass, of carbon in the hydrocarbon? Hint: Use moles to relate the quantities of the two substances.

Accepted Answer

The answer of A 4.626 g sample of a hydrocarbon,...

Question 6

In a quantitative analysis study, 4.624 grams of a hydrocarbon compound yielded 13.84 g of CO₂ and 7.556 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Accepted Answer

The moles of carbon in CO₂ and hydrogen in H₂O are calculated and compared to find the simplest whole number ratio. The moles of carbon are 13.84 g CO₂ / 44.01 g/mol = 0.3145 mol C. The moles of hydrogen are 7.556 g H₂O / 18.02 g/mol = 0.419 mol H, which is 0.838 mol H (since each H₂O has 2 H atoms). The ratio of C:H is approximately 3:8, leading to the empirical formula C₃H₈.

Question 7

In a quantitative analysis study, 2.644 grams of a hydrocarbon compound yielded 8.008 g of CO₂ and 4.098 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Accepted Answer

The answer of In a quantitative analysis study, 2.644 grams...

Question 8

In a quantitative analysis study, 4.624 grams of a compound containing carbon, hydrogen and oxygen yielded 6.557 g of CO₂ and 4.026 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Accepted Answer

The answer of In a quantitative analysis study, 4.624 grams...

Question 9

In a quantitative analysis study, 1.878 grams of a compound containing carbon, hydrogen and oxygen yielded 3.258 g of CO₂ and 1.778 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Accepted Answer

The answer of In a quantitative analysis study, 1.878 grams...

Question 10

Magnesium reacts with aqueous hydrochloric acid to give an aqueous solution of magnesium chloride and hydrogen gas. Select the correct balanced chemical equation for this reaction.

Accepted Answer

The balanced chemical equation for the reaction of magnesium with hydrochloric acid is Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g), where one magnesium atom reacts with two hydrochloric acid molecules to produce one magnesium chloride molecule and one hydrogen gas molecule.

Question 11

Select the correct balanced chemical equation for the reaction below. C₆H₁₄ + O₂ $\rarr$ CO₂ + H₂O

Accepted Answer

The balanced equation is 2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O, which balances the number of carbon, hydrogen, and oxygen atoms on both sides.

Question 12

When BaCl₂ reacts with Na₃PO₄, the products formed are Ba₃(PO₄)₂ and NaCl. How many moles of Ba₃PO₄ are formed for each mole of BaCl₂ that is consumed?

Accepted Answer

The balanced chemical equation is 3BaCl2 + 2Na3PO4 → Ba3(PO4)2 + 6NaCl. For every 3 moles of BaCl2, 1 mole of Ba3(PO4)2 is formed, so for each mole of BaCl2, 1/3 or 0.3333 moles of Ba3(PO4)2 are formed.

Question 13

Given: 3H₂(g)+ N₂(g)s 2NH₃(g)If the reaction begins with 0.500 mol of H₂, how many atoms of hydrogen in the compound NH₃would you expect to make?

Accepted Answer

The answer of Given: 3H₂(g)+ N₂(g)s 2NH₃(g)If the reaction begins...

Question 14

Select the correct balanced chemical equation. Hint: Distribute coefficients across the entire formula they apply to and be sure to correctly calculate the number of atoms inside the parentheses.

Accepted Answer

The answer of Select the correct balanced chemical equation. Hint:...

Question 15

In the chemical reaction C₂H₆O + PCl₃ $\rarr$C₂H₅Cl + H₃PO₃, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

Accepted Answer

The answer of In the chemical reaction C₂H₆O + PCl₃...

Question 16

In the chemical reaction C₂H₆O + SOCl₂ $\rarr$ C₂H₅Cl + H₂SO₃, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

Accepted Answer

The balanced equation is C2H6O + SOCl2 → C2H5Cl + H2SO3. The coefficients are 1 for each compound, so the sum is 1 + 1 + 1 + 1 = 4.

Question 17

Given the following chemical equation: S + NaOH $\rarr$ Na₂SO₃ + Na₂S + H₂O,the coefficient in front of NaOH should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

Accepted Answer

The balanced equation is 3S + 6NaOH → Na2SO3 + 2Na2S + 3H2O, so the coefficient in front of NaOH is 6.

Question 18

When ethene (C₂H₄)is burned in the presence of oxygen gas, the products are carbon dioxide and water. When balanced with the smallest set of whole numbers, the coefficient for the oxygen gas molecule is

Accepted Answer

The answer of When ethene (C₂H₄)is burned in the presence...

Question 19

Thermal decomposition of KClO₃(s)yields KCl(s)and O₂(g). When 4.289 grams of KClO₃ undergo this reaction, how many grams of oxygen gas are produced? Hint: Write and balance the equation first, then do the stoichiometric calculations.

Accepted Answer

The answer of Thermal decomposition of KClO₃(s)yields KCl(s)and O₂(g). When...

Question 20

When aluminum metal reacts with HCl(aq), the products formed are AlCl₃(aq)and the hydrogen gas molecule. If 4.288 grams of Al (0.1590 moles)undergo this reaction with an excess of hydrochloric acid, how many grams of hydrogen gas should be produced? Hint: Write and balance the equation first, then do the stoichiometric calculations.

Accepted Answer

The answer of When aluminum metal reacts with HCl(aq), the...

Quiz 4: The Mole and Stoichiometry

A compound contains potassium, sulfur, and oxygen. The composition of the compound is: potassium, 49.410%; sulfur, 20.261%. Determine the empirical formula of the compound. Hint: Assume you have 100 grams of this substance and use moles to relate the mass of one element to another.

A 4.626 g sample of a hydrocarbon, upon combustion analysis, yielded 6.484 grams of carbon dioxide. What is the percent, by mass, of carbon in the hydrocarbon? Hint: Use moles to relate the quantities of the two substances.

In a quantitative analysis study, 4.624 grams of a hydrocarbon compound yielded 13.84 g of CO₂ and 7.556 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 2.644 grams of a hydrocarbon compound yielded 8.008 g of CO₂ and 4.098 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 4.624 grams of a compound containing carbon, hydrogen and oxygen yielded 6.557 g of CO₂ and 4.026 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 1.878 grams of a compound containing carbon, hydrogen and oxygen yielded 3.258 g of CO₂ and 1.778 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Magnesium reacts with aqueous hydrochloric acid to give an aqueous solution of magnesium chloride and hydrogen gas. Select the correct balanced chemical equation for this reaction.

Select the correct balanced chemical equation for the reaction below. C₆H₁₄ + O₂ $\rarr$ CO₂ + H₂O

When BaCl₂ reacts with Na₃PO₄, the products formed are Ba₃(PO₄) ₂ and NaCl. How many moles of Ba₃PO₄ are formed for each mole of BaCl₂ that is consumed?

Given: 3H₂(g) + N₂(g) s 2NH₃(g) If the reaction begins with 0.500 mol of H₂, how many atoms of hydrogen in the compound NH₃would you expect to make?

Select the correct balanced chemical equation. Hint: Distribute coefficients across the entire formula they apply to and be sure to correctly calculate the number of atoms inside the parentheses.

In the chemical reaction C₂H₆O + PCl₃ $\rarr$ C₂H₅Cl + H₃PO₃, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

In the chemical reaction C₂H₆O + SOCl₂ $\rarr$ C₂H₅Cl + H₂SO₃, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

Given the following chemical equation: S + NaOH $\rarr$ Na₂SO₃ + Na₂S + H₂O,the coefficient in front of NaOH should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

When ethene (C₂H₄) is burned in the presence of oxygen gas, the products are carbon dioxide and water. When balanced with the smallest set of whole numbers, the coefficient for the oxygen gas molecule is

Thermal decomposition of KClO₃(s) yields KCl(s) and O₂(g) . When 4.289 grams of KClO₃ undergo this reaction, how many grams of oxygen gas are produced? Hint: Write and balance the equation first, then do the stoichiometric calculations.

Quiz 4: The Mole and Stoichiometry

A compound contains potassium, sulfur, and oxygen. The composition of the compound is: potassium, 49.410%; sulfur, 20.261%. Determine the empirical formula of the compound. Hint: Assume you have 100 grams of this substance and use moles to relate the mass of one element to another.

A 4.626 g sample of a hydrocarbon, upon combustion analysis, yielded 6.484 grams of carbon dioxide. What is the percent, by mass, of carbon in the hydrocarbon? Hint: Use moles to relate the quantities of the two substances.

In a quantitative analysis study, 4.624 grams of a hydrocarbon compound yielded 13.84 g of CO2 and 7.556 g of H2O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 2.644 grams of a hydrocarbon compound yielded 8.008 g of CO2 and 4.098 g of H2O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 4.624 grams of a compound containing carbon, hydrogen and oxygen yielded 6.557 g of CO2 and 4.026 g of H2O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 1.878 grams of a compound containing carbon, hydrogen and oxygen yielded 3.258 g of CO2 and 1.778 g of H2O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Magnesium reacts with aqueous hydrochloric acid to give an aqueous solution of magnesium chloride and hydrogen gas. Select the correct balanced chemical equation for this reaction.

Select the correct balanced chemical equation for the reaction below. C6H14 + O2 →\rarr→ CO2 + H2O

When BaCl2 reacts with Na3PO4, the products formed are Ba3(PO4) 2 and NaCl. How many moles of Ba3PO4 are formed for each mole of BaCl2 that is consumed?

Given: 3H2(g) + N2(g) s 2NH3(g) If the reaction begins with 0.500 mol of H2, how many atoms of hydrogen in the compound NH3 would you expect to make?

Select the correct balanced chemical equation. Hint: Distribute coefficients across the entire formula they apply to and be sure to correctly calculate the number of atoms inside the parentheses.

In the chemical reaction C2H6O + PCl3 →\rarr→ C2H5Cl + H3PO3, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

In the chemical reaction C2H6O + SOCl2 →\rarr→ C2H5Cl + H2SO3, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

Given the following chemical equation: S + NaOH →\rarr→ Na2SO3 + Na2S + H2O,the coefficient in front of NaOH should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

When ethene (C2H4) is burned in the presence of oxygen gas, the products are carbon dioxide and water. When balanced with the smallest set of whole numbers, the coefficient for the oxygen gas molecule is

Thermal decomposition of KClO3(s) yields KCl(s) and O2(g) . When 4.289 grams of KClO3 undergo this reaction, how many grams of oxygen gas are produced? Hint: Write and balance the equation first, then do the stoichiometric calculations.

In a quantitative analysis study, 4.624 grams of a hydrocarbon compound yielded 13.84 g of CO₂ and 7.556 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 2.644 grams of a hydrocarbon compound yielded 8.008 g of CO₂ and 4.098 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 4.624 grams of a compound containing carbon, hydrogen and oxygen yielded 6.557 g of CO₂ and 4.026 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

In a quantitative analysis study, 1.878 grams of a compound containing carbon, hydrogen and oxygen yielded 3.258 g of CO₂ and 1.778 g of H₂O in a combustion analysis apparatus. Determine the empirical formula of the compound. Hint: Use moles to relate the quantities of the substances.

Select the correct balanced chemical equation for the reaction below. C₆H₁₄ + O₂ $\rarr$ CO₂ + H₂O

When BaCl₂ reacts with Na₃PO₄, the products formed are Ba₃(PO₄) ₂ and NaCl. How many moles of Ba₃PO₄ are formed for each mole of BaCl₂ that is consumed?

Given: 3H₂(g) + N₂(g) s 2NH₃(g) If the reaction begins with 0.500 mol of H₂, how many atoms of hydrogen in the compound NH₃would you expect to make?

In the chemical reaction C₂H₆O + PCl₃ $\rarr$ C₂H₅Cl + H₃PO₃, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

In the chemical reaction C₂H₆O + SOCl₂ $\rarr$ C₂H₅Cl + H₂SO₃, when the equation is balanced, the sum of the coefficients of the reactants and products should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

Given the following chemical equation: S + NaOH $\rarr$ Na₂SO₃ + Na₂S + H₂O,the coefficient in front of NaOH should be: Hint: Distribute coefficients across the entire formula they apply to when calculating atoms.

When ethene (C₂H₄) is burned in the presence of oxygen gas, the products are carbon dioxide and water. When balanced with the smallest set of whole numbers, the coefficient for the oxygen gas molecule is

Thermal decomposition of KClO₃(s) yields KCl(s) and O₂(g) . When 4.289 grams of KClO₃ undergo this reaction, how many grams of oxygen gas are produced? Hint: Write and balance the equation first, then do the stoichiometric calculations.