The molar mass of water (h2o) is 18.0 g/mol. a sample of water has a mass of 18.0 g. how many moles of water are contained in this sample?
a) 1.00
b) 18.0
c) 36.0
d) 324

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2