Limiting Reactants and Percent Yield

What is a limiting reactant?

• The reactant that is present in excess and does not limit the reaction.

• The substance that is completely consumed in a chemical reaction, limiting the amount of product that can be formed.

• The reactant that determines the rate of the reaction.

• The product formed in the highest quantity during a reaction.

What is the balanced equation for the reaction of magnesium and hydrochloric acid?

• Mg + HCl → MgCl + H2

• Mg + 2HCl → MgCl2 + H2

• Mg + HCl → MgCl2 + H2

• Mg + 2HCl → MgCl2 + Cl2

What is actual yield?

• The theoretical amount of product expected from a reaction.

• The amount of product that is actually obtained from a chemical reaction, measured after the experiment.

• The total amount of reactants used in a chemical reaction.

• The amount of product that could be produced if all reactants were converted to products.

In the reaction 4NH3 + 5O2 → 4NO + 6H2O, how many grams of NO are formed from 6.30 g of NH3?

• 1.35 g of NO is formed.

• 2.50 g of NO is formed.

• 0.75 g of NO is formed.

• 3.00 g of NO is formed.

How do you identify the limiting reactant in a reaction?

• By calculating the moles of each reactant and determining which one produces the least amount of product.

• By adding excess reactant to ensure complete reaction.

• By measuring the temperature change during the reaction.

• By observing the color change of the reactants.

What is the significance of the limiting reactant in a chemical reaction?

• It determines the maximum amount of product that can be formed and affects the efficiency of the reaction.

• It is the reactant that is present in excess and does not limit the reaction.

• It is the reactant that is consumed first and has no effect on the reaction rate.

• It is the reactant that is used to speed up the reaction without being consumed.

How do you convert grams of a reactant to moles?

• Moles = Mass (g) / Molar Mass (g/mol)

• Moles = Mass (g) x Molar Mass (g/mol)

• Moles = Molar Mass (g/mol) / Mass (g)

• Moles = Mass (g) + Molar Mass (g/mol)

How much SOCl2 is produced from 16.2 g of SO2 and 13.7 g of PCl5?

• 5.00 g of SOCl2

• 6.50 g of SOCl2

• 7.83 g of SOCl2

• 9.10 g of SOCl2

How do you calculate percent yield?

• (Actual Yield / Theoretical Yield) x 100%

• (Theoretical Yield / Actual Yield) x 100%

• (Actual Yield + Theoretical Yield) x 100%

• (Actual Yield - Theoretical Yield) x 100%

What is the percent yield if the theoretical yield is 12.3 g and the actual yield is 10.1 g?

• 70.5%

• 75.0%

• 82.1%

• 90.0%