A lighter contains 3.59 g of butane. How many moles of butane are present at STP?

Thoughts: So, correct me if I'm wrong however is it appropriate just to calculate its molar mass, and then use that molar mass and the given mass to figure out moles??

Yes, mols = grams/molar mass. By the way, it doesn't matter whether the gas is at STP or any other pressure/temperature combinations, the fact is that 3.59 g is so many moles regardless of the pressure/temperature.

Thank you so much!! I assumed that was the case :)

I noticed you used different screen names of Gerry and Bob. It helps us help you better if you stick with the same name.

Yes, you're on the right track! To determine the number of moles of butane present at STP (Standard Temperature and Pressure), you can follow these steps:

1. Calculate the molar mass of butane (C₄H₁₀):
- The molar mass of carbon (C) is 12.01 g/mol, and there are four carbon atoms in butane.
- The molar mass of hydrogen (H) is 1.01 g/mol, and there are ten hydrogen atoms in butane.
- Multiply the molar mass of carbon by 4 and the molar mass of hydrogen by 10, then sum them together to get the molar mass of butane.

2. Use the molar mass of butane to find the number of moles:
- Divide the given mass (3.59 g) by the molar mass of butane.
- This calculation will give you the number of moles of butane present at STP.

Remember to use the same unit for mass and molar mass (either grams or moles) to ensure correct results.