# Combustion of a 0.9827 g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of #CO_2# and 1.070 g of #H_2O#. What is the empirical formula of the compound?

##### 2 Answers

#### Answer:

The empirical formula is

#### Explanation:

Here is the equation with masses:

Use 32.00 g/mol for the molar mass of

Use 18.03 g/mol for the molar mass of

Use 44.01 g/mol for the molar mass of

We do not know the molar mass of the hydrocarbon so we allow

Perform the division:

Matching coefficients, we get:

Divide every number by 0.02149:

Multiply every number by 2:

Round off each number to the nearest integer.

The empirical formula is

#### Answer:

The empirical formula is

#### Explanation:

First, we calculate the masses of

This is less than the mass of the sample.

The missing mass must be caused by

Now, we must convert these masses to moles and find their ratios.

From here on, I like to summarize the calculations in a table.

The **empirical formula** is

**Note**: This is an impossible empirical formula.

The molecular formula must have an even number of

A compound with 8