when 79.0 g of calcium and 54.7 g of nitrogen gas undergo a reaction that has a 90.9% yield, what mass of calcium nitride forms?
__________g calcium nitride
3Ca + N2 ------------> Ca3N2
Now, molar mass of Ca = 40 g/mole
molar mass of N2 = 28 g/mole
moles of 79 g of Ca = 79/40 = 1.975
moles of 54.7 g of N2 = 54.7/28 = 1.954
Now, as per the balanced reaction:- Ca and N2 reacts in the ratio of 3:1
Thus, for 1.954 moles of N2 , 5.862 moles of Ca is required
Clearly, Ca is the limiting reagent
Thus, theoretical yield of Ca3N2 = (1/3)*moles of Ca = (1/3)*1.975 = 0.6583 moles
Theoretical yield of Ca3N2 in grams = 0.6853*148 = 97.43 g
Actual yield of Ca3N2 = 0.909*97.43 = 88.57 g
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