Education • All: 3.6: Limiting Reactant

LIMITING REACTANT

Given the mass (grams) of each reactant determine the amount of product that can be produced from each reaction.

Example:

Question 1: Given 2.00 grams of zinc (Zn) and 2.50 grams of silver nitrate (AgNO3), which one is the liming reactant?

Balanced Equation:

Zn (s) + 2AgNO3 ---> 2Ag + Zn(NO3)2

Step 1

Find how many grams of Silver (Ag) can be obtained with 2.00 grams of zinc (Zn)

$\large \fn_cm \\2.00\;g\;Zn\times \frac{1\;mol\;Zn}{63.5\;g\;Zn}\times \frac{2\;mol\;Ag}{1\;mol\;Zn}\times \frac{107.9\;g\;Ag}{1\;mol\;Ag}={\color{Purple} 6.80\;g\;Ag}$

Step 2

Find how many grams of Silver (Ag) can be obtained with 2.50 grams of Silver Nitrate (AgNO3)

$\dpi{120} \fn_cm \\2.50\;g\;AgNO_{3}\times \frac{1\;mol\;AgNO_{3}}{169\;g\;AgNO_{3}}\times \frac{2\;mol\;Ag}{2\;mol\;AgNO_{3}}\times \frac{107.9\;g\;Ag}{1\;mol\;Ag}={\color{Purple} 1.59\;g\;Ag}$

Step 3

Compare my results. The one that produces the least amount of product, is the limiting reactant.

2.00 grams of Zinc produces 6.80 grams of product

2.50 grams of Silver Nitrate produces 1.59 grams of product

The liming reactant is Silver Nitrate

Question 2: How much Zinc was used to produce the 1.59 grams of Silver?

$\dpi{120} \fn_cm \\1.59\;g\;Ag\times \frac{1\;mol\;Ag}{107.9\;g\;Ag}\times \frac{1\;mol\;Zn}{2\;mol\;Ag}\times \frac{65.4\;g\;Zn}{1\;mol\;Zn}={\color{Purple} 0.48\;g\;Zn}$

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3.6: Limiting Reactant

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