How many moles of H2O are produced when 64.0 g C2H2 burns in oxygen

1 answer:

6 0

The balanced chemical reaction will be:

C2H2 + 5/2O2 = 2CO2 + H2O

We are given the amount of C2H2 being burned. This will be our starting point.

64.0 g C2H2 (1 mol C2H2 / 26.02 g C2H2) (1 mol H2O/1mol C2H2) ( 18.02 g H2O/1mol H2O) = 44.32 g H2O.

Thus, the answer is 44.32 g H2O.

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