Question

- How many grams of H2 are needed to produce 14.48 g of NH3?

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- How many molecules (not moles) of NH3 are produced from 6.59×10⁻⁴ g of H2?

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Answer 1

As we know N2 + 3H2 ------> 2NH3

the reaction specify that 3 moles of H2 are required to produce 2 moles of NH3 or we can say to produce 2 mole of NH3 , 3 moles of H2 is rrequired.

moles NH3 = 14.48 g/17.0307 g/mol=0.8502
moles H2 = 0.8502 x 3 /2=1.275
mass H2 = 1.275 mol x 2 g/mol= 2.55 grams

b) From the above equation

No. of moles H2 = 6.59 X 10^-4 g / 2 g = 3.295 X 10^-4
No. of moles NH3 = 3.295 X 10^-4 x 2 /3 = 2.196 X 10^-4
No. of molecules of NH3 = 2.196 X 10^-4 x 6.02 x 10^23 = 13.223 X 10^-19