How many grams of #H_2# are needed to produce 13.68g of #NH_3#?

1 Answer
anor277
Feb 23, 2016

We need (i) the molar quantity of ammonia, and (ii) a stoichiometric equation that shows ammonia synthesis.

Explanation:

#"Moles of ammonia"# #=# #(13.68*g)/(17.03*g*mol^-1)# #=# #0.803# #mol.#

#1/2N_2(g) + 3/2H_2(g) rarr NH_3(g)#

From the stoichiometry, we know that there are 1.5 moles dihydrogen required for each mole of ammonia. There we require #1.21# #mol# dihydrogen.

#"Mass of dihydrogen" = 1.21 *molxx2.02*g*mol^-1# #=# #??# #g#.

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