Question

16. For the equation 2CH. +90, 6CO2 + 6H2O, 43.3 grams of CH is reacted with 520 grums Os. If the reaction proceeds via a 60.6% yield, how many grams of H.O will fom?

Answer 1

This is a simple question

For this we have to find the theroretical yield first

And then find it's 60.6% to know exact answer

We have reaction

2C₃H₆ + 9O₂ ---> 6H₂O

So according to stoichiometric ratio for every 2 moles of C₃H₆ and 9 moles of O₂ 6 moles of H₂O is produced

We have

43.3 grams of C₃H₆

So no of moles = weight/molar mass

= 43.3/42.08

=1.028

And we have 52.0 grams of O2

Moles = weight/molar mass

52/32

= 1.625 moles

Since the C₃H₆ and O₂ have relationship of 2:9

Not all moles of C3H6 will be used

No of moles of C₃H₆ used will be

(1.625/9) ×2

0.3611 moles

Similarly theoretical yield of H2O will be

(1.625/9) ×6

1.0833 moles of H₂O

1 mole of H₂O = 18.01

So 1.0833×18.01

= 19.51 gram

Since this is 100% yield

60.6% yield =

19.51× (60.6/100)

= 11.82 gram of H₂O will be produced

I hope this helps. If you have any query or want more detailed explanation, feel free to ask in the comments section below.