1.44 g H2 is allowed to react with 9.56 g N2, producing 2.46 g NH3. What...

1.44 g H2 is allowed to react with 9.56 g N2, producing 2.46 g NH3.

What is the theoretical yield?

What is the percent yield?

Expert Solution

The balenced chemical reaction is:

3H2 + N2 <---------> 2NH3

ie. 6g of H2 must react with 28g of N2 to produce 34g of NH3

the available H2 = 1.44g and N2 = 9.56g and product NH3 = 2.46g

the limiting factor here is H2

So, Theoretical yield will be decided by the presence of H2 (ie. limiting factor)

Theoretical yield = wt of H2 consumed x 34 / 6

= 1.44 x 34 / 6

= 8.16% (100% yield). This is the amount of NH3 in gram, should have formed after complete consumption of 1.44g of H2.

but, obtained amount is = 2.46g of NH3 only.

Now, percentage yield = 2.46 x 100 / 8.16

= 30.14%

perc

queen_honey_blossom answered 2 years ago

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