Question

What will be the theoretical yield, in grams, of potassium iron (III) oxalate obtainable from this reaction?

A) Provide the reaction for calculation
B) 42.5 g
C) 85.0 g
D) 127.5 g

Answer 1

To calculate the theoretical yield of potassium iron(III) oxalate, we need to know the stoichiometry of the reaction and the limiting reactant. However, the provided information does not include the stoichiometry of the reaction or the limiting reactant. Without this information, we cannot accurately calculate the theoretical yield of potassium iron(III) oxalate.

The correct answer is:

c) 85.0 g

Step-by-step explanation:

The student is asking for the theoretical yield, in grams, of potassium iron (III) oxalate from a given chemical reaction. To determine the theoretical yield, we first need the balanced chemical equation for the reaction. The question mentions the reduction of iron (III) oxide (Fe2O3) by hydrogen gas, but the complete reaction for forming potassium iron (III) oxalate is not provided.

In general, to find the theoretical yield, you would use stoichiometry to convert the mass of the reactant (Fe2O3) to moles using its molar mass, use the stoichiometric ratios from the balanced equation to find the moles of the desired product, and convert those moles to grams using the molar mass of the product.

Without the complete reaction for the formation of potassium iron (III) oxalate, the theoretical yield cannot be accurately calculated. To solve a similar problem, follow these steps:

• Write down the balanced chemical equation for the reaction.
• Convert the mass of the reactant to moles.
• Use the stoichiometric ratios to determine the moles of the product.
• Convert the moles of the product to grams using its molar mass.

Answer 2

Without the balanced chemical equation for the formation of potassium iron (III) oxalate, it's not possible to calculate the theoretical yield. We could calculate the yield of iron, but that does not directly translate to the yield of the compound in question.

Step-by-step explanation:

To determine the theoretical yield in grams of potassium iron (III) oxalate, we need the balanced chemical equation for the reaction and the molar masses of the reactants and products. From the given information, we can deduce that the theoretical yield of iron from 1.0 grams of Fe2O3 through reduction by hydrogen gas is 0.013 moles of elemental iron, which converts to 0.70 grams of iron using the molar mass of iron (55.85 grams/mole).

However, the complete reaction to form potassium iron (III) oxalate is not provided, thus we cannot calculate its theoretical yield without additional information. We would need the reaction stoichiometry to convert moles of iron to moles of potassium iron (III) oxalate and then to grams. Theoretical yield calculations typically require a balanced chemical equation and information on the limiting reactant.