Question 1: A mole is a unit used to measure the amount of substance in chemistry. It allows scientists to count particles, such as atoms or molecules, by relating them to a standard number. Why is the concept of a mole important when discussing fuels and emissions in automobiles?

Answer: The mole allows scientists to quantify the number of molecules involved in fuel combustion and emissions, making it easier to calculate and compare chemical reactions in engines.

Question 1: Define a mole in terms of particles, and state the number of particles in one mole.

Answer: A mole is a quantity that contains 6.022 x 10^23 particles (atoms, molecules, or ions).

Question 2: Explain why understanding moles is useful when analyzing the amount of sulfur dioxide (SO2) produced by a car's emissions.

Answer: Because it allows for precise calculation of the number of SO2 molecules emitted, which is important for environmental impact assessments.

Question 1: Calculate the number of moles in 44 grams of carbon dioxide (CO2). (Molecular weight of CO2 = 44 g/mol)

Answer: Number of moles = mass / molar mass = 44 g / 44 g/mol = 1 mol

Question 2: A car's catalytic converter reduces 0.5 moles of nitrogen oxides (NOx) emissions. How many molecules of NOx are emitted? (Use Avogadro's number: 6.022 x 10^23 molecules/mol)

Answer: Number of molecules = 0.5 mol x 6.022 x 10^23 molecules/mol = 3.011 x 10^23 molecules

Question 1: Design a simple experiment to measure the amount of carbon monoxide (CO) produced by a small engine. List the variables that need to be controlled and safety precautions that should be taken.

Answer: Students should outline collecting exhaust gases in a secure container, controlling engine speed and fuel type, ensuring proper ventilation, and wearing safety goggles and gloves to prevent exposure to toxic gases.

Question 1: A vehicle emits 2.5 grams of sulfur dioxide (SO2). Given that the molar mass of SO2 is 64 g/mol, how many moles of SO2 were emitted? What does this tell you about the number of molecules released?

Answer: Moles of SO2 = 2.5 g / 64 g/mol ≈ 0.0391 mol; Number of molecules = 0.0391 mol x 6.022 x 10^23 ≈ 2.35 x 10^22 molecules

Question 1: Explain how understanding moles and chemical reactions helps automotive engineers design cleaner engines and reduce emissions.

Answer: By calculating the amounts of reactants and products in chemical reactions, engineers can optimize fuel combustion, improve catalytic converter efficiency, and develop technologies that minimize harmful emissions.

Question 1: A vehicle consumes 50 liters of gasoline, which has an approximate density of 0.75 g/mL. The chemical formula of gasoline is complex, but on average, 1 mole of gasoline (approximated as octane, C8H18) weighs about 114 g. Calculate the total moles of octane in the consumed gasoline. How does this relate to the number of molecules involved in combustion? (Show all steps and reasoning.)

Answer: Mass of gasoline = 50 L x 1000 mL/L x 0.75 g/mL = 37,500 g. Moles of octane = 37,500 g / 114 g/mol ≈ 328.95 mol. Number of molecules = 328.95 mol x 6.022 x 10^23 ≈ 1.98 x 10^26 molecules. This illustrates the vast number of molecules involved in fuel combustion and highlights the importance of mole calculations in industry.