Asked by Tyler
Calculate the number of hydrogen molecules formed when 5.6 mL of ammonia at STP is decomposed by the following reaction:
___NH3 „³ ___ N2 + ___ H2
___NH3 „³ ___ N2 + ___ H2
Answers
Answered by
bobpursley
ammonia gas?
You will have to know the temp,pressure to convert that volume to moles, then to molecules.
Recommend balance the equation first.
You will have to know the temp,pressure to convert that volume to moles, then to molecules.
Recommend balance the equation first.
Answered by
Graham
You have 5.6 mL of NH3.
There are 22.4 L per mole of gas at STP.
So 5.6e-3 / 22.4 mole of NH3.
Balance the equation to determine the corresponding number of H2.
There are 22.4 L per mole of gas at STP.
So 5.6e-3 / 22.4 mole of NH3.
Balance the equation to determine the corresponding number of H2.
Answered by
bobpursley
Correct, Graham, I missed the STP statement.
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.