1. A website promoting the use of alternative energy vehicles and hybrid technologies claims that, \"A typical automobile in the USA uses about 500 gallons of gasoline every year, producing about 5 tons of carbon dioxide.\"

To determine the truth of this statement, calculate how many tons of carbon dioxide are produced when 500.0 gallons of gasoline are combusted. Assume that the primary ingredient in gasoline is octane, C8H18(l), which has a density of 0.703 g·mL–1.

2. Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 5.021 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich environment. The products of the combustion were 5.465 g of CO2(g) and 2.796 g of H2O(g). Insert subscripts below to appropriately display the empirical formula of the gasoline additive:

Any help is really appreciated!

To answer these questions, we need to use some basic chemistry concepts, such as stoichiometry, molecular formulas, and empirical formulas. Let's go step by step.

1. To calculate the amount of carbon dioxide produced when 500.0 gallons of gasoline are combusted, we need to know the molecular formula of octane (C8H18) and use stoichiometry.

Step 1: Convert the volume of gasoline (in gallons) to mass (in grams).
Since we know the density of octane, we can calculate the mass of 500.0 gallons of gasoline:
Mass = Volume x Density
Mass = 500.0 gallons x (3.785 L/gallon) x (1000 mL/L) x (0.703 g/mL)

Step 2: Determine the molar mass of octane.
To do this, we need to calculate the molar mass of each element in octane and sum them up.
Molar mass of carbon (C) = 12.01 g/mol
Molar mass of hydrogen (H) = 1.008 g/mol

Molar mass of octane (C8H18) = (8 x 12.01 g/mol) + (18 x 1.008 g/mol)

Step 3: Use the balanced chemical equation for combustion of octane to determine the moles of carbon dioxide produced.
The balanced chemical equation for the combustion of octane is:
C8H18 + 12.5 O2 -> 8 CO2 + 9 H2O
From this equation, we can see that 8 moles of CO2 are produced for every mole of octane consumed.

Step 4: Convert the mass of gasoline to moles using the molar mass of octane.
Moles of octane = Mass of gasoline / Molar mass of octane

Step 5: Use the mole ratio between octane and carbon dioxide to calculate the moles of carbon dioxide produced.
Moles of CO2 = Moles of octane x (8 moles CO2 / 1 mole octane)

Step 6: Calculate the mass of carbon dioxide produced.
Mass of CO2 = Moles of CO2 x Molar mass of CO2

Finally, divide the mass of CO2 by 1000 to convert it into tons.

2. To determine the empirical formula of the gasoline additive, we need to use the information given about the combustion products.

Step 1: Calculate the moles of carbon dioxide (CO2) and water (H2O) produced.
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of H2O = Mass of H2O / Molar mass of H2O

Step 2: Determine the moles of carbon and hydrogen in the sample.
Moles of carbon = Moles of CO2 (from step 1)
Moles of hydrogen = Moles of H2O (from step 1)

Step 3: Convert the moles of carbon and hydrogen to whole numbers by dividing by the smallest number of moles.
Divide the moles of carbon and hydrogen by the smaller of the two. Round the ratios to the nearest whole number.

The resulting whole numbers represent the subscripts of carbon (C), hydrogen (H), and possibly any other elements present in the additive. The empirical formula is displayed using these subscripts.

I hope this explanation helps you understand how to solve these problems!