Question #421e4
1 Answer
True.
Explanation:
The key here is the balanced chemical equation that describes the formation of water from hydrogen gas and oxygen gas
#2"H"_ (2(g)) + "O"_ (2(g)) -> 2"H"_ 2"O"_ ((l))#
Two things to notice here
#color(blue)((1))# . The number of moles of water produced by the reaction is equal to the number of moles of hydrogen gas consumed by the reaction#-># the two chemical species are in a#2:2# mole ratio.
#color(blue)((2))# . The reaction consumes#2# moles of hydrogen gas for very#1# mole of oxygen gas that takes part in the reaction#-># the two reactants are in a#2:1# mole ratio.
In your case, you know that you are mixing
According to
In other words, hydrogen gas will act as the limiting reagent, i.e. it will be completely consumed before all the moles of oxygen gas will get the chance to react.
So if the reaction consumes
Therefore, you can say that the affirmation is true--when
You can add to this by saying that