### All SAT II Chemistry Resources

## Example Questions

### Example Question #1 : Empirical And Molecular Formulas

Vanillin is composed of carbon, oxygen, and hydrogen.

What is the empirical formula of vanillin?

Refer to the following table for the atomic masses of the elements shown:

**Possible Answers:**

**Correct answer:**

In order to calculate the empirical formula of vanillin from the given percent composition data, we can pretend we have a 100 g sample vanillin and from there estimate how many grams of each element make up the sample. For example, Vanillin is carbon; therefore, the estimated sample would contain 66.3 g of carbon. After doing this for each of the elements vanillin contains, we can use the atomic mass of carbon to find how many moles of carbon make up the sample. We then do the same for each element that composes vanillin. See calculations below:

After finding the number of moles of each element in the hypothetical 100 g sample, we look at the ratio between the moles of each element by dividing all the samples by smallest number of moles. After finding the ratios of the samples, we are able to use the empirical formula of the vanillin by rounding up to the nearest whole number for each sample. If the ratios are not close enough to round up (like in this example), we multiply the ratios all by the same number until each number is equal to a whole number nicely. See calculations below:

We need whole numbers, so multiply each of the resulting numbers by 3 to get rid of the fractions.

This gives us as the final answer.

### Example Question #1 : Empirical And Molecular Formulas

Which pair of formulas represents the empirical formula and molecular formula for a certain compound?

**Possible Answers:**

**Correct answer:**

To find an empirical formula, take a molecular formula and divide the subscript of each element by the greatest common factor of all the subscripts. In this case, the only pair that works is , which can be verified by dividing the coefficients of the molecular formula by 6. Note that is not correct because neither of the formulas is an empirical formula; they are both possible molecular formulas for a compound with the empirical formula .

### Example Question #1 : Stoichiometry

What is the approximate percentage of carbon by mass in heptane, which has the molecular formula ?

**Possible Answers:**

**Correct answer:**

First, calculate the molar mass of heptane, which is

We can calculate the percentage of carbon by mass in heptane by creating a fraction of the mass of carbon over the mass of the entire molecule and converting it into a percentage:

For every 100 g of heptane, 84 g must come from carbon. This means that the percentage of carbon by mass is

### Example Question #1 : Stoichiometry

How many nitrate ions are in one mole of ?

**Possible Answers:**

**Correct answer:**

Note that there are two nitrate () ions for every formula unit of calcium nitrate. This means that in one mole of calcium nitrate, there are two moles of nitrate ions. To go from moles to ions, multiply 2 by Avogadro's number.

### Example Question #1 : Stoichiometry

How many hydrogen atoms are in one mole of ?

**Possible Answers:**

**Correct answer:**

In one molecule of , there are 2 ammonium ions, each of which has 4 hydrogen atoms for a total of 8 hydrogen atoms. Thus, to find the number of hydrogen atoms in one mole of , one must multiply Avogadro's number by 8.

### Example Question #1 : Stoichiometry

Calculate the number of aluminum ions in moles of _{.}

**Possible Answers:**

**Correct answer:**

In order calculate the number of aluminum ions, we must first find the number of aluminum ions in the entire compound. In this case, there are two molecules of ^{ } for every molecule of . After understanding this, we can use Avogadro's constant to determine the number of atoms (more specifically ions) of aluminum. See equation below for specific calculations.

### Example Question #1 : Avogadro's Number

How many atoms of chloride are in 0.2550 g of aluminum chloride, ?

**Possible Answers:**

**Correct answer:**

The formula for aluminum chloride is . The molar mass of is 26.98 g and the molar mass of is 35.45 g. There are three atoms in . To calculate the molecular mass of , we need to find the sum of the mass of one aluminum atom and three chlorine atoms:

The total molecular weight is 130.33 g. Starting with the grams of , we convert to the amount of moles using the molecular weight value we just calculated. Then we calculate the number of moles of chloride ion in . using the 3:1 ratio. Finally, we calculate the number of atoms by using Avogadro's number. See calculations below:

### Example Question #1 : Stoichiometry

When the equation for the reaction shown below is balanced with the lowest whole-number coefficients, what is the sum of the coefficients of the reactants?

___ ___ ___ ___

**Possible Answers:**

**Correct answer:**

The coefficients of the equation, when balanced, should be 2, 13, 10, and 8. This problem wants to know the sum of the *reactants*, so only the coefficients on the left side of the reactants should be added. The sum of 2 and 13 is 15, so 15 is the correct answer.

### Example Question #2 : Stoichiometry

Suppose that 8 grams of of hydrogen gas and 16 grams of oxygen gas are ignited. What is the theoretical yield, in grams, of water? Assume hydrogen has an atomic mass of 1 and oxygen has an atomic mass of 16.

**Possible Answers:**

**Correct answer:**

First, convert from grams to moles using the molar masses of the compounds. There are 4 mol of hydrogen gas and 0.5 mol of oxygen gas. Oxygen gas is clearly the limiting reagent (since there is more than twice as much hydrogen gas as oxygen gas), which means that the theoretical yield of water is

Water contains two hydrogen atoms and an oxygen atom, so it has a molar mass of

Hence, 1 mol of water would have a mass of 18 g.

### Example Question #1 : Stoichiometry With Reactions

Octane, , is an important of component of gasoline, which can be burned as fuel in cars. The following is an *unbalanced* equation for the combustion of octane.

If 114 g of octane are burned in the complete combustion reaction shown below, how many grams of water will be produced?

___ ___ ___ ___

**Possible Answers:**

**Correct answer:**

First, the equation should be balanced. This can be done with the coefficients 2, 25, 16, and 18.

Next, calculating the molar mass of octane shows that it has a molar mass of 114 g/mol. This means that 1 mole of octane is used in the reaction, and 9 times as many moles of water should be produced, meaning one of the products will be 9 mol of water. Water has a molar mass of 18 g/mol, so the total mass of water produced is .

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