Optional Stoichiometry Review

Front

What is percent yield in a chemical reaction?

Back

Percent yield is the ratio of the actual yield (the amount of product obtained) to the theoretical yield (the maximum amount of product that could be formed) expressed as a percentage.

Front

How do you calculate percent yield?

Back

Percent Yield = (Actual Yield / Theoretical Yield) x 100%

Tags

NGSS.HS-PS1-7

Front

What is a limiting reactant?

Back

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

Front

What happens when the limiting reactant is used up?

Back

When the limiting reactant is used up, the chemical reaction stops because there are no more reactants available to continue the reaction.

Front

What is theoretical yield?

Back

Theoretical yield is the maximum amount of product that can be produced from a given amount of reactants, calculated based on stoichiometric ratios.

Tags

NGSS.HS-PS1-7

Front

What is actual yield?

Back

Actual yield is the amount of product that is actually obtained from a chemical reaction, which is often less than the theoretical yield due to various factors.

Front

What is the mole ratio in a balanced chemical equation?

Back

The mole ratio is the ratio of moles of one substance to the moles of another substance in a balanced chemical equation, used to convert between moles of reactants and products.

Tags

NGSS.HS-PS1-7

Front

For the reaction 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe, what is the mole ratio of Mg to Fe?

Back

The mole ratio of Mg to Fe is 3 mol Mg / 2 mol Fe.

Tags

NGSS.HS-PS1-7

Front

What is the significance of balancing a chemical equation?

Back

Balancing a chemical equation ensures that the law of conservation of mass is obeyed, meaning the number of atoms of each element is the same on both sides of the equation.

Tags

NGSS.HS-PS1-7

Front

What does it mean if a reaction has a low percent yield?

Back

A low percent yield indicates that the reaction was not efficient, possibly due to incomplete reactions, side reactions, or loss of product during recovery.

Tags

NGSS.HS-PS1-6