Asked by Gerry

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??
Answered by DrBob222
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.
Answered by Gerry
Thank you so much!! I assumed that was the case :)
Answered by DrBob222
I noticed you used different screen names of Gerry and Bob. It helps us help you better if you stick with the same name.
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