For the haber process, n2+3h2 yields 2nh3, what volume of nitrogen is consumed at stp if you collect 44.8 l of ammonia in excess hydrogen (n=14 amu, h=1 amu)
a. 14.9 l
b. 29.9 l
c. 44.8l
d. 22.4 l

d. 22.4 L

Explanation:

According to Avogadro's law , 1 mole of every gas occupies 22.4 L of volume at STP.

moles of ammonia=

Given: Hydrogen is the excess reagent and nitrogen is the limiting reagent as it limits the formation of product.

From the given balanced equation:

2 moles of ammonia is produced by 1 mole of nitrogen.

Thus 2 moles of ammonia is produced by 22.4 L of nitrogen at STP as 1 mole of nitrogen occupies 22.4 L at STP.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

the answer is 75.0%.