What is the volume, in liters, of 11.6 g of ethane gas (C_2H_6) at STP? Round your answer to 3 significant figures.

• A. 22.4 L
• B. 11.2 L
• C. 8.70 L
• D. 5.80 L

Answer: (C)

Verified step by step guidance

1. Identify the molar mass of ethane (C\_2H\_6) by summing the atomic masses of its atoms: 2 carbons and 6 hydrogens. Use the atomic masses approximately 12.01 g/mol for carbon and 1.008 g/mol for hydrogen.
2. Calculate the number of moles of ethane using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\), where the mass is 11.6 g and the molar mass is from step 1.
3. Recall that at STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters.
4. Calculate the volume of ethane gas by multiplying the number of moles by 22.4 L/mol: \(\text{volume} = \text{moles} \times 22.4 \text{ L/mol}\).
5. Round the final volume to 3 significant figures as requested.