Chapter 5 - Mastering Chemistry

The number of moles of NaOH that are in 250 mL of a 3.0 molar solution is 0.25 moles. 0.75 moles. 1.0 moles. 1.5 moles.

0.75 moles

When the equation is balanced, Zn + CuSO4 → ZnSO4 + Cu, the coefficient of copper is: 0 1 2 3

1

How many moles of sulfur atoms are present in 0.500 moles of CS2? 1.00 4.00 0.500 0.250

1.00

Which of the following has the same number of atoms as 35.4 g of chlorine? 19 g of potassium 18 g of water 35.4 g germanium 12 g of carbon

12 g of carbon

Which of the following does NOT contain Avogadro's number of particles? 12 g of water 1.0 mole of silver 6.02 × 1023 atoms of aluminum 23 g of sodium

12 g of water

Octane (C8H18 ) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). When the equation is balanced, C8H18 + O2 → CO2 + H2O, the coefficient of octane is: 25 16 8 2

2

The following reaction is important in the removal of sulfur dioxide, a major source of acid rain, from the smokestacks of coal burning power plants. When the equation is balanced, CaO + SO2 + O2 → CaSO4, the coefficient of calcium oxide (commonly called "lime") is: 1 2 3 4

2

When oxygen, O2, is passed through an electrical spark (lightning is a good natural source of an electrical spark), ozone, O3, is formed. When the equation is balanced, the coefficient of ozone is 1 2 3 4

2

When the equation is balanced, Fe + O2 → Fe2O3, the coefficient of the product is: 1 2 3 4

2

Which one of the following reactions is NOT balanced? 2 CO + O2 → 2 CO2 2 SO2 + O2 → 2 SO3 SF4 + 3 H2O → H2SO3 + 4 HF 2 KNO3 + 10 K → 5 K2O + N2

2 KNO3 + 10 K → 5 K2O + N2

Express the chemical equation in terms of moles. 2C4H10+13O2 → 8CO2+10H2O 2 moles of butane (C4H10) react with 13 moles of oxygen (O2) to produce 8 moles of carbon dioxide (CO2) and 10 moles of water (H2O). 2 moles of butane (C4H10) react with 13 moles of oxygen (O2) to produce 8 moles of carbon dioxide (CO2) and 8 moles of water (H2O). 2 moles of butane (C4H10) react with 26 moles of oxygen (O2) to produce 8 moles of carbon dioxide (CO2) and 10 moles of water (H2O). 2 moles of butane (C4H10) react with 8 moles of oxygen (O2) to produce 13 moles of carbon dioxide (CO2) and 10 moles of water (H2O).

2 moles of butane (C4H10) react with 13 moles of oxygen (O2) to produce 8 moles of carbon dioxide (CO2) and 10 moles of water (H2O).

Express the chemical equation in terms of moles. 2Mg+O2 → 2MgO 1 mole of magnesium (Mg) reacts with 1 mole of oxygen (O2) to produce 1 mole of magnesium oxide (MgO). 1 mole of magnesium (Mg) reacts with 1 mole of oxygen (O2) to produce 1 mole of magnesium oxide (MgO). 2 moles of magnesium (Mg) react with 1 mole of oxygen (O2) to produce 2 moles of magnesium oxide (MgO). 2 moles of magnesium (Mg) react with 2 moles of oxygen (O2) to produce 2 moles of magnesium oxide (MgO).

2 moles of magnesium (Mg) react with 1 mole of oxygen (O2) to produce 2 moles of magnesium oxide (MgO).

Describe how you would prepare 2.44 kg of an aqueous solution that is 16.3% KOH by mass. 0.163 kg KOH. Add 0.163 kg KOH to 2.277 kg water. 0.163 kg KOH. Add 0.163 kg KOH to 2.603 kg water. 2.44 kg solution x 0.163 = 0.40 kg KOH. Add 0.40 kg KOH to 2.84 kg water. 2.44 kg solution x 0.163 = 0.40 kg KOH. Add 0.40 kg KOH to 2.04 kg water.

2.44 kg solution x 0.163 = 0.40 kg KOH. Add 0.40 kg KOH to 2.04 kg water.

The molarity of a solution that contains 0.50 moles of NaOH in 200.0 milliliters of water is 0.25 M. 0.5 M. 1.0 M. 2.5 M.

2.5 M

How many moles of (NH4)2S are there in 200 g of (NH4)2S? 1.84 2.94 4.17 4.00

2.94

Nitroglycerin has a formula C3H5(NO3)3. The molar mass of nitroglycerin is 65 g/mole. 227 g/mole. 309 g/mole. 398 g/mole.

227 g/mole

What is the molar mass of P4O8? 311.8 g/mol 12 251.9 g/mol 251.9 amu

251.9 g/mol

Consider the following balanced reaction: 2 SO2(g) + O2(g) → 2 SO3(g) What is the ratio of volumes for SO2, O2, and SO3, respectively? 1:1:1 6:2:8 2:0:2 2:1:2

2:1:2

What is the molarity of a potassium iodide solution prepared from 0.400 mol of KI in 125 mL of solution? 0.00320 M 0.313 M 0.0500 M 3.20 M

3.20 M

Acetylene (C2H2) burns in pure oxygen with a very hot flame. The products of this reaction are carbon dioxide and water. How much oxygen is required to react with 13.0 g of acetylene? 13.0 g 40.0 g 8.00 g 60.0 g

40.0g

Avogadro's number is: 6.02 × 10^23 6.02 × 10^-23 2.06 × 10^32 3.02 × 10^26

6.02 x 10^23

What is the mass of 0.500 mol of NH3? 34.0 g 8.50 g 3.40 g 7.50 g

8.5

Which of the following is correct, according to Avogadro's hypothesis? At 0°C and 1 atm pressure, equal volumes of gases contain equal masses. At 0°C and 1 atm pressure, equal volumes of gases contain the same number of molecules. At 0°C and 1 atm pressure, 1 L of oxygen gas and 1 L of liquid water contain the same number of molecules. At 0°C and 1 atm pressure, equal volumes of gases have the same density.

At 0°C and 1 atm pressure, equal volumes of gases contain the same number of molecules.

concentrated solution Solution with a large quantity of solute dissolved in a small quantity of solvent. Solution with a small quantity of solute dissolved in a large quantity of solvent. Solution with a small quantity of solute dissolved in a small quantity of solvent. Solution with a large quantity of solute dissolved in a large quantity of solvent. dilute solution Solution with a large quantity of solute dissolved in a small quantity of solvent. Solution with a small quantity of solute dissolved in a large quantity of solvent. Solution with a small quantity of solute dissolved in a small quantity of solvent. Solution with a large quantity of solute dissolved in a large quantity of solvent. soluble A substance that cannot be dissolved by the solvent. A substance that can be dissolved in a large quantity of solvent. A substance that can be dissolved by the solvent. A substance that cannot be dissolved in a small quantity of solvent. insoluble A substance that cannot be dissolved by the solvent. A substance that can be dissolved in a large quantity of solvent. A substance that can be dissolved by the solvent. A substance that cannot be dissolved in a small quantity of solvent.

Solution with a large quantity of solute dissolved in a small quantity of solvent. Solution with a small quantity of solute dissolved in a large quantity of solvent. A substance that can be dissolved by the solvent.

The molarity (M) of a solution is the number of moles of solute per liter of solution. True False

True

Consider 1.00 molH2(g), 2.00 molHe(g), and 0.50 molC2H2(g) at the same temperature and pressure. Part A: Do the three samples have the same number of atoms? Yes, the three samples have the same number of atoms. No, three samples have no identical number of atoms. Part B: Which sample has the greatest mass? H2 He C2H2

Yes, the three samples have the same number of atoms. C2H2

A solution is made from 5.0 g of glucose (C6H12O6), 10.0 g of table salt (NaCl), and 85.0 g of ethanol (C2H5OH). Which substance(s) is the solvent? View Available Hint(s) ethanol glucose glucose + table salt table salt

ethanol

A solution that is 1 molar contains six moles of solute in 6 moles of solvent. six moles of solute in 600 g of solution. five moles of solute in 5 moles of solution. four moles of solute in 4 liters of solution.

four moles of solute in 4 liters of solution.

A chemist dissolves 9 g of NaCl in 225 mL of water. Water is the solution. solubility. solute. solvent.

solvent

According to Avogadro's hypothesis, equal volumes of gases at the same temperature and pressure will have the same number of molecules. True False

true

The reactants are the starting materials in a reaction. True False

true

The stoichiometric factor relates the moles of any two substances in a balanced chemical reaction. True False

true