Using the equation below, how many grams of co2 are produced when 54.5g of c2h2 is burned?

2c2h2 + 5o2 --> 4co2 + 2h2o

The answer to your question is 92.23 g of CO₂

Explanation:

                    2C₂H₂   +   5O₂   ⇒   4CO₂   +   2H₂O

Process

1.- Calculate the molecular mass of C₂H₂ and CO₂

Molecular mass C₂H₂ = (12 x 2) + (1 x 2) = 24 + 2 = 26 g

Molecular mass CO₂ = (12 x 1) + (16 x 2) = 12 + 32 = 44g

2.- The balance reaction and proportion to find the amount of CO₂ produced.

                    2(26) g of C₂H₂  4(44) g of CO₂

                     54.5 g of C₂H₂   x

                     x = (54.5 x 88) / 52

                    x = 92.23 g of CO₂