Answer:
Based on the search results [1], [3], and [6], the calculation to determine the empirical formula of butane gas if it consists of 81.82% carbon and 18.18% hydrogen is:
Step 1: Assume 100 g of the compound, so there are 81.82 g of carbon and 18.18 g of hydrogen.
Step 2: Convert the mass of each element to moles using their molar masses.
- Carbon: 81.82 g C × (1 mol C/12.01 g C) = 6.82 mol C
- Hydrogen: 18.18 g H × (1 mol H/1.01 g H) = 18.0 mol H
Step 3: Divide each amount of moles by the smallest number of moles to get the simplest whole-number ratio.
- Carbon: 6.82 mol C ÷ 6.82 = 1 mol C
- Hydrogen: 18.0 mol H ÷ 6.82 = 2.64 mol H ≈ 3 mol H
Step 4: Write the empirical formula using the integers found in the previous step.
- The empirical formula of butane gas with 81.82% carbon and 18.18% hydrogen is CH3.
Therefore, the empirical formula of butane gas when it contains 81.82% carbon and 18.18% hydrogen is CH3.
Step-by-step explanation: