Quantitative Chem 2 Flashcards
(20 cards)
What is percentage yield?
(Actual yield ÷ Theoretical yield) × 100.
What does a low percentage yield mean?
Not all reactants were converted into products.
Give one reason why yield might be less than expected.
Loss during transfer, side reactions, or incomplete reactions.
What is theoretical yield?
The maximum possible amount of product based on the balanced equation.
What is actual yield?
The mass of product actually obtained from a reaction.
What is concentration?
The amount of solute in a given volume of solution.
What is the formula for concentration (g/dm³)?
Concentration = Mass of solute ÷ Volume of solution (dm³).
How do you convert cm³ to dm³?
Divide by 1000.
What is the formula for concentration in mol/dm³?
Concentration = Moles ÷ Volume (dm³).
What is the formula for moles in solution?
Moles = Concentration × Volume (dm³).
How many cm³ are in 1 dm³?
1000 cm³.
What volume does 1 mole of gas occupy at room temperature and pressure (RTP)?
24 dm³.
What is the formula for gas volume?
Volume = Moles × 24 (at RTP).
How can you calculate moles of gas from volume?
Moles = Volume (dm³) ÷ 24.
What does RTP stand for?
Room Temperature and Pressure.
What is a limiting reactant?
The reactant that is completely used up in a reaction, stopping the reaction.
What is an excess reactant?
The reactant left over after the reaction is complete.
Why is it important to identify the limiting reactant?
Because it determines the maximum amount of product formed.
How do you identify the limiting reactant from moles?
Compare mole ratios from the balanced equation with moles available.
What happens if the limiting reactant runs out?
The reaction stops and no more product is formed.
