Calculating the Amount of Product Formed

Chapter , Problem 1PE

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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 \(\mathrm {H_2}\)?

When 24 mol of methanol and 15 mol of oxygen combine in the combustion reaction \(2\ \mathrm{CH}_{3} \mathrm{OH}(l)+3\ \mathrm{O}_{2}(g) \longrightarrow 2\ \mathrm{CO}_{2}(g)+4\ \mathrm{H}_{2} \mathrm{O}(g)\), what is the excess reactant and how many moles of it remains at the end of the reaction?
(a) 9 mol \(\mathrm {CH_3OH}(l)\), (b) 10 mol \(\mathrm {CO_2}(g)\), (c) 10 mol \(\mathrm {CH_3 OH}(l)\), (d) 14 mol \(\mathrm {CH_3 OH}(l)\), (e) 1 mol \(\mathrm {O_2}(g)\).

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 CH_{3}OH(l)+3 O_{2}(g){rightarrow}2 CO_{2}(g)+4 H_{2}O(g)

CH_{3}OH(l)

CO_{2}(g)

CH_{3}OH(l)

CH_{3}OH(l)

O_{2}(g)