When 28.0 g of acetylene reacts with hydrogen, 24.5 g of ethane is produced. What is the perce

step 1 If our chemical reaction is C2H2 reacting with hydrogen, two moles of hydrogen, to produce C2H6

When 28.0 g of acetylene reacts with hydrogen, 24.5 g of...

When $28.0 \mathrm{~g}$ of acetylene reacts with hydrogen, $24.5 \mathrm{~g}$ of ethane is produced. What is the percent yield of $\mathrm{C}_{2} \mathrm{H}_{6}$ for the reaction? $(9.2,9.3,9.5)$ $$ \mathrm{C}_{2} \mathrm{H}_{2}(g)+2 \mathrm{H}_{2}(g) \stackrel{\mathrm{Pt}}{\longrightarrow} \mathrm{C}_{2} \mathrm{H}_{6}(g) $$

When $28.0 \mathrm{~g}$ of acetylene reacts with hydrogen, $24.5 \mathrm{~g}$ of ethane is produced. What is the percent yield of $\mathrm{C}_{2} \mathrm{H}_{6}$ for the reaction? $(9.2,9.3,9.5)$
$$
\mathrm{C}_{2} \mathrm{H}_{2}(g)+2 \mathrm{H}_{2}(g) \stackrel{\mathrm{Pt}}{\longrightarrow} \mathrm{C}_{2} \mathrm{H}_{6}(g)
$$

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Key Concepts

Actual Yield

The actual yield is the measured amount of product obtained from an experiment or reaction. It reflects the real-world outcome, which can be lower than the theoretical yield due to factors such as incomplete reactions or practical inefficiencies.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction. It is calculated by dividing the actual yield by the theoretical yield and multiplying by 100, thereby indicating the proportion of the expected product that was actually produced.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant, calculated using stoichiometry under the assumption that the reaction goes to completion without any losses.

Stoichiometry

Stoichiometry involves using a balanced chemical equation to determine the quantitative relationships between reactants and products in a chemical reaction. It allows the calculation of how much of each reactant is needed and how much product will form, often involving conversions between mass and moles.

Molar Mass

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole. It is critical for converting between the mass given in a problem and the number of moles, which is necessary for making stoichiometric calculations.

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