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??
3 answers
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.
2 answers