Question

what is the theoretical yield of amonia (in grams) if 17.15 grams of nitrogen gas and 10.95 grams of hydrogen gas are allowed to react? show dimensial analysis.

Answer 1

N2 + 3H2 ---------------> 2NH3 MOLE = MASS / MOLECULAR MASS

17.15 GM N2 MOLE OF NITROGEN = 17.15/ 28 = 0.6125 MOLE MOLECULAR MASS OF N2 = 28

10.95 GM OF H2 , MOLE OF HYDROGEN = 10. 95 / 2 = 5.475 MOLE MOLECULAR MASS OF H2 = 2

NOW OBSERVING THE REACTION WE FOUND THAT 1 MOLE OF NITROGEN REACTS WITH 3 MOLE OF HYDROGEN ...

SO 0.6125 * 3 = 1.8375 MOLE HYDROGEN WILL CONSUME AND REMAINING HYDROGEN WILL LEFT

SO AMMONIA WILL PRODUCE ....ONCE AGIAN WATCHING THE REACTION 1 MOLE N2 PRODUCE 2 MOLE OF NH3 . HERE NITROGEN IS LIMITING REAGENT

SO AMMONIA = 2 * 0.6125 = 1.225 MOLE

MOLECULAR MASS OF AMMONIA = 17

TOTAL MASS OF AMMONIA = 17 * 1.225 = 20.825 G

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