1.10 is allowed to react with 9.57 , producing 2.50 .

What is the theoretical yield for this reaction under the given conditions?

no units.

To determine the theoretical yield for a reaction, you need to compare the stoichiometry of the reactants and products. The stoichiometry is the balanced ratio of moles between reactants and products in the reaction equation.

From the given information, you know that 1.10 moles of one reactant react with 9.57 moles of another reactant to produce 2.50 moles of the product.

To find the theoretical yield, you need to determine the limiting reactant. The limiting reactant is the one that is completely consumed in the reaction and determines the maximum amount of product that can be formed.

To find the limiting reactant, you can compare the moles of reactants used to their stoichiometric ratio. In this case, you need to compare the moles of the two reactants.

Let's assume the balanced equation is:

aA + bB ā†’ cC

Where A and B are the reactants, C is the product, and a, b, and c are the stoichiometric coefficients.

Based on the given information, you can set up the following ratio:

1.10 (moles of A) / a = 9.57 (moles of B) / b

Solving for a/b, you get:

a/b = (1.10 / 9.57)

Compare this ratio to the stoichiometric coefficients in the balanced equation to determine the limiting reactant.

Once you identify the limiting reactant, you can calculate the theoretical yield by using the stoichiometric coefficients:

Theoretical yield = (moles of limiting reactant) * (stoichiometric coefficient of the product)

For example, if A is the limiting reactant and its stoichiometric coefficient is a, then the theoretical yield would be:

Theoretical yield = 1.10 (moles of A) * (stoichiometric coefficient of C)

If B is the limiting reactant and its stoichiometric coefficient is b, then the theoretical yield would be:

Theoretical yield = 9.57 (moles of B) * (stoichiometric coefficient of C)