How many grams of #N_2# are required to completely react with 3.03 grams of #H_2# for the equation #N_2 + 3H_2 -> 2NH_3#?

1 Answer
Dec 10, 2015

Answer:

#7.01"g"#

Explanation:

Notice the coefficients of #N_2# and #H_2#.

Since the equation has an #N_2# and #3H_2#, #3# times as many moles of #H_2# will be used as #N_2# assuming a complete reaction.

Since we're given the mass of #H_2# being used, we can divide that by the molar mass of #H_2# to determine how many moles of #H_2# will be consumed. We can divide that mole amount by #3# to find how many moles of #N_2# the reaction will use, and multiply that by the molar mass of #N_2# to find how many grams we should use.

#3.03"g"H_2xx(1"mol"H_2)/(2.02"g"H_2)xx(1"mol"N_2)/(3"mol"H_2)xx(14.02"g"N_2)/(1"mol"N_2)=7.01"g"N_2#