Question

How much C2H4N2 could be expected from the reaction of13.5 g CO2,2.23 g NH3, and1.63 g CH4?

Answer 1

Balance chemical equation:---

3CH4 + 5CO2 + 8NH3 --> 4C2H4N2 + 10H2O

Moles of CO2 = 13.5/44 = 0.3068 mol

Moles of NH3 = 2.23/17= 0.1312 mol

Moles of CH4= 1.63/16 = 0.1019 mol

For complete reaction of NH3, CH4 required = 0.1312*(3/8) = 0.0492 mol , CO2 required= 0.1312*(5/8) = 0.082

But here CO2 and CH4 both present in excess hence NH3 is the limiting reagent.

Now, moles of C2H4N2 produced = 0.1312*(4/8) = 0.0656 mol

Mass of C2H4N2 = moles x molar mass

0.0656 x 56 = 3.6736 gram.

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