How many grams of co₂ will be produced from 7.00 g of c₃h₈ and 98.0 g of o₂?

The answer to your question is  21 g of CO₂  

Explanation:

Balanced Reaction

                               C₃H₈  +  6O₂    ⇒    3CO₂   +   4H₂O

Data

mass of C₃H₈ = 7 g

mass of O₂  = 98 g

Determine the limiting reactant

Molecular mass of C₃H₈ = (12 x3) + (1 x 8) = 36 + 8 = 44 g

Molecular mass of Oxygen = 16 x 12 = 192 g

Theoretical proportion  C₃H₈ / O₂ = 44 / 192 = 0.23

Experimental proportion  C₃H₈ / O₂ = 7 / 98 = 0.07

As the proportion diminishes in the experiment, the excess reagent is the oxygen and the limiting reactant is propane.

- Calculate the mass of CO₂

                     44 g of C₃H₈   3(44) of CO₂

                       7 g of C₃H₈       x

                       x = (7 x 3(44)) / 44

                       x = 924 / 44

                       x = 21 g of CO₂                        

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

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