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How many grams of the first reactant in each of the following chemical

equations would be needed to produce 49.7 g of N2 gas?

(a) 4NH3 + 3O2 → 2N2 + 6H2O

 = ? g of NH3

(b) (NH4)2Cr2O7 → N2 + 4H2O + Cr2O3

 = ? g of (NH4)2Cr2O7

(c) N2H4 + 2H2O2 → N2 + 4H2O

= ? g of N2H4

(d) 2NH3 → N2 + 3H2

= ? g of NH3

Top Answer

Given mass of N 2 = 49.7 g Molecular mass of N2 = 2(14.0067) =28.0134 which is equivalent to 28 g/mole So, no of moles of N2... View the full answer

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