Final answer:
The percent yield of acetylene (C2H2) from water (H2O) in the reaction is calculated by dividing the actual yield by the theoretical yield and then multiplying by 100%. The actual yield is given as 41.5g, but without the balanced reaction and molar masses, we cannot calculate the theoretical yield or the percent yield.
Step-by-step explanation:
The percent yield of a chemical reaction can be calculated using the formula: Percent Yield = (Actual Yield / Theoretical Yield) × 100%.
In the given reaction, the reactant is water (H2O) and the product is acetylene (C2H2). To calculate the theoretical yield of C2H2, we would need to use stoichiometry based on the balanced equation, which is missing in the question. However, the actual yield has been provided as 41.5g.
If we had the balanced equation and the molar masses of reactants and products, we could calculate the moles of C2H2 that should be produced from 49.8g of water, which would give us the theoretical yield. Using the actual yield and the theoretical yield, we could then calculate the percent yield.
For example, if a theoretical yield of 50g is calculated, then the percent yield would be (41.5g / 50g) × 100% = 83%.