Concept explainers
Interpretation:
The percent yield has to be calculated for the given reaction, if
Concept Introduction:
The mass of a product isolated from a reaction is known as the actual yield. The actual yield of a product, the result of a laboratory experiment is less than the theoretical yield and is expressed as percent yield.
Limiting reactant:
Limiting reactant is the one that yields the smallest amount of any one product. If the mass of more than one reactant is given, approach the stoichiometry problem by calculating the number of moles of product formed from the quantity of each reactant. The reactant that yields the smallest amount of product is limiting; use it for the stoichiometry calculation.
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Chemistry: Principles and Practice
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- When sprayed into the flame of a torch, powdered iron reacts with oxygen from the air to form iron(III) oxide, Fe2O3: 4 Fe(s) + 3 O02(g) → 2 Fe2O3(s) If 2.50 g Fe2O3 is formed by this reaction, calculate the maximum total mass of iron metal and oxygen that reacted. Identify the stoichiometric coefficients in this equation. If 10,000 oxygen atoms reacted, calculate how many Fe atoms were needed to react with this quantity of oxygen.arrow_forwardThe sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)arrow_forwardThe catalytic converter that is standard equipment on American automobiles converts carbon monoxide (CO)to carbon dioxide (CO2) by the reaction 2CO + O2 2CO2 What mass of O2, in grams, is needed to react completely with 25.0 g of CO?arrow_forward
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