Asked by Bradley

What mass of water, in grams, would have to be decomposed to produce 13.3 L of molecular oxygen at STP?

How do I go about doing this problem?

Answers

Answered by bobpursley
how many moles is that?

n=PV/RT solve that.

Then, each mole of water decomposes to 1/2 mole of oxygen gas. so whatever moles of O2 you found, multipy by two, that is the moles of water, convert that to grams.
There are no AI answers yet. The ability to request AI answers is coming soon!

Related Questions