REG Limiting Reactant & % Yield

CH₄  +  2O₂  →  CO₂  +  2H₂O
1.50 grams of CH₄ was added to the above reaction. Calculate the theoretical yield of CO₂ in grams.

(MM of CO₂ = 44.01 g/mol)

• 66 grams
• 132 grams
• 33 grams
• 8.72

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

• Percent
• actual
• stoichiometry
• theoretical

Tags

NGSS.HS-PS1-6

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

• 90.4%

• 104%

• 96.15%

• 1.04%

2Fe₂O₃ + 3C → 4Fe + 3CO₂

You add 2.33 mol of Carbon to the reaction. You find the actual yield to be 2.98 mol of Fe.

What is the percent yield of Fe?

(Hint: calculate theoretical yield of moles of Fe first)

• 95.9%

• 128%

• 78.2%

• 58.6%

• 170%

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

• 1.16%
• 116%
• 85%
• 76%

​ (a)   is what is produced in lab while ​ (b)   is what is calculated.

• Actual yield
• theoretical yield
• reactant
• product
• limiting reactant

A student is trying to figure out the problem below:

2O2 + CH4 → CO2 + 2H2O

5.0 moles of water are produced. How many grams of methane (CH4) were used?

What is wrong with the student's set up?

Tags

NGSS.HS-PS1-7

NGSS.HS-PS1-2

Where do you get the molar mass from?

• periodic table

• coefficients in the reaction

• you just have it memorized

• it is always one

• I don't know

Tags

NGSS.HS-PS1-1

Where do you get the mole ratio from?

• periodic table

• coefficients in the reaction

• you just have it memorized

• it is always one

• I don't know

Tags

NGSS.HS-PS1-7

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

• Limiting Reactant

• Excess Reactant

• Highly Reactant

• Super Reactant