Question

The combustion of propyne $\left(\mathrm{C}_{3} \mathrm{H}_{4}\right)$ releases heat when it burns according to the following equation: $(7.6,7.7,7.8)$ $$ \mathrm{C}_{3} \mathrm{H}_{4}(g)+4 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) $$ a. How many moles of $\mathrm{O}_{2}$ are needed to react completely with $0.225$ mole of $\mathrm{C}_{3} \mathrm{H}_{4}$ ? b. How many grams of water are produced from the complete reaction of $64.0 \mathrm{~g}$ of $\mathrm{O}_{2}$ ? c. How many grams of $\mathrm{CO}_{2}$ are produced from the complete reaction of $78.0 \mathrm{~g}$ of $\mathrm{C}_{3} \mathrm{H}_{4}$ ? d. If the reaction in part e produces $186 \mathrm{~g}$ of $\mathrm{CO}_{2}$, what is the percent yield of $\mathrm{CO}_{2}$ for the reaction?

          The combustion of propyne $\left(\mathrm{C}_{3} \mathrm{H}_{4}\right)$ releases heat when it burns according to the following equation: $(7.6,7.7,7.8)$
$$
\mathrm{C}_{3} \mathrm{H}_{4}(g)+4 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{O}_{2}$ are needed to react completely with $0.225$ mole of $\mathrm{C}_{3} \mathrm{H}_{4}$ ?
b. How many grams of water are produced from the complete reaction of $64.0 \mathrm{~g}$ of $\mathrm{O}_{2}$ ?
c. How many grams of $\mathrm{CO}_{2}$ are produced from the complete reaction of $78.0 \mathrm{~g}$ of $\mathrm{C}_{3} \mathrm{H}_{4}$ ?
d. If the reaction in part e produces $186 \mathrm{~g}$ of $\mathrm{CO}_{2}$, what is the percent yield of $\mathrm{CO}_{2}$ for the reaction?

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Added by Brittany M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

07/05/2023

Step 1

From the balanced chemical equation, we can see that 1 mole of $\mathrm{C}_{3} \mathrm{H}_{4}$ reacts with 4 moles of $\mathrm{O}_{2}$. Show more…

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The combustion of propyne $left(mathrm{C}_{3} mathrm{H}_{4} ight)$ releases heat when it burns according to the following equation: $$ mathrm{C}_{3} mathrm{H}_{4}(g)+4 mathrm{O}_{2}(g) stackrel{Delta}{longrightarrow} 3 mathrm{CO}_{2}(g)+2 mathrm{H}_{2} mathrm{O}(g) $$ a. How many moles of $mathrm{O}_{2}$ are needed to react completely with $0.225$ mole of $mathrm{C}_{3} mathrm{H}_{4}$ ? b. How many grams of water are produced from the complete reaction of $64.0 mathrm{~g}$ of $mathrm{O}_{2}$ ? c. How many grams of $mathrm{CO}_{2}$ are produced from the complete reaction of $78.0 mathrm{~g}$ of $mathrm{C}_{3} mathrm{H}_{4}$ ? d. If the reaction in part e produces $186 mathrm{~g}$ of $mathrm{CO}_{2}$, what is the percent yield of $mathrm{CO}_{2}$ for the reaction?

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