Consider the following reaction: 2 NO(g) + 5 H2(g) ? 2 NH3(g) + 2 H2O(g) Which s

Question

Consider the following reaction: 2 NO(g) + 5 H2(g) ? 2 NH3(g) + 2 H2O(g) Which set of solution maps would be needed to calculate the maximum amount of ammonia (NH3), in grams, that can be synthesized from 45.8 g of nitrogen monoxide (NO) and 12.4 g of hydrogen (H2)? I. g NO ? mol NO ? mol NH3 ? g NH3 II. g H2 ? mol H2 ? mol NH3 ? g NH3 III. g NO ? mol NO ? mol H2O ? g H2O IV. g H2 ? mol H2 ? mol H2O ? g H2O. solutions maps I and II solutions maps I and V solutions maps I and III solutions maps II and III

Explanation / Answer

Given for the reaction,

moles NO = 45.8 g/30 g/mol = 1.53 moles

moles H2 = 12.4 g/2 g/mol = 6.2 moles

Limiting reactant = NO

theoretical maximum yield (100%) for NH3 = 1.53 moles x 17 g/mol = 26.01 g

So maximum yield map would be,

I. g NO -->mol NO --> mol NH3 --> g NH3

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