Calculating the Amount of Product Formed

Chapter , Problem 2PE

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Calculating the Amount of Product Formed from a Limiting Reactant

The most important commercial process for converting \(\mathrm {N_2}\) from the air into nitrogen-containing compounds is based on the reaction of \(\mathrm {N_2}\) and \(\mathrm {H_2}\) to form ammonia \(\left(\mathrm{NH}_{3}\right)\):

\(\mathrm{N}_{2}(g)+3\ \mathrm{H}_{2}(g) \longrightarrow 2\ \mathrm{NH}_{3}(g)\)

How many moles of \(\mathrm {NH_3}\) can be formed from 3.0 mol of \(\mathrm {N_2}\) and 6.0 mol of \(\mathrm {H_2}\)?

(a) When 1.50 mol of Al and 3.00 mol of \(\mathrm {Cl_2}\) combine in the reaction \(2\ \mathrm{Al}(s)+3\ \mathrm{Cl}_{2}(g) \longrightarrow 2\ \mathrm{AlCl}_{3}(s)\), which is the limiting reactant? (b) How many moles of \(\mathrm {AlCl_3}\) are formed? (c) How many moles of the excess reactant remain at the end of the reaction?

Equation Transcription:

Text Transcription:

N_2

N_2

N_2

(NH3)

N_{2}(g)+3 H2(g)2 NH3(g)

NH3

N_2

H_2

2 Al(s)+3 Cl_{2}(g){rightarrow}2 AlCl_{3}(s)

AlCl+{3}