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?
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.
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!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.