Question

PLEASE HELP ASAP

A total of 132.33g C3H8 is burned in 384.00 g O2. Use the following questions to determine the amounts of products formed.
• How many grams of CO2 and H2O will be produced? (2 points)
















b. If the furnace is not properly adjusted, the products of combustion can include other gases, such as CO and unburned hydrocarbons. If only 269.34 g of CO2 were formed in the above reaction, what would the percent yield be? (2 points)

Answer 1

To determine the amounts of CO2 and H2O produced when burning C3H8 and O2, we balance the combustion reaction equation and use stoichiometry. The percent yield can be calculated if the actual yield of CO2 is known.

Step-by-step explanation:

To determine the amounts of CO2 and H2O produced when burning C3H8 and O2, we need to balance the combustion reaction equation and use stoichiometry. The equation is C3H8 + 5O2 → 3CO2 + 4H2O. Using the molar masses of C3H8 and O2, we can calculate the moles of each reactant. From the balanced equation, we know that the molar ratio of C3H8 to CO2 is 1:3 and the molar ratio of C3H8 to H2O is 1:4. Using these ratios, we can convert the moles of C3H8 to grams of CO2 and H2O.

If only 269.34 g of CO2 were formed in the reaction, we can calculate the moles of CO2 produced. Then, we can determine the theoretical yield of CO2 based on the balanced equation. The percent yield can be calculated by dividing the actual yield (269.34 g) by the theoretical yield and multiplying by 100.

Answer 2

A combustion reaction takes place in the presence of O2 (g). The
products of a complete combustion reaction are CO2 (g) and H2O
(g).