Solved: Limiting Reactants (Section)One of the steps in
Chapter , Problem 80E(choose chapter or problem)
Limiting Reactants (Section 3.7)
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of \(\mathrm {NH_3}\) to NO:
\(\mathrm {4\ NH_3}(g)+5\ \mathrm O_2(g) \longrightarrow 4\ \mathrm NO(g)+6\ \mathrm {H_2O}(g)\)
In a certain experiment, of \(\mathrm{NH}_{3}\) reacts with 2.50 g of \(\mathrm O_2\). (a) Which is the limiting reactant? (b) How many grams of NO and \(\mathrm {H_2O}\) form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.
Equation Transcription:
Text Transcription:
NH_3
NO
4 NH_{3}(g)+5 O_{2}(g){rightarrow}4 NO(g)+6 H_{2}O(g)
NH_3
O_2
NO
H_{2}O
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