A sample of a diatomic gas is loaded into a bottle at STP. The 0.25 L bottle contains 1.76 grams of the gas. Calculate the molar mass of the gas and identify what kind of gas it is.

Tin has ten stable isotopes. the heaviest, 124sn, makes up 5.80% of naturally occuring tin atoms. how many atoms of 124sn are present in 82.0 g of naturally occurring tin? what is the total mass of the 124sn atoms in this sample?

Define dew point. i am writing this part to be able to ask the question

How many moles of oxygen gas are produced from the decomposition of six moles of potassium