Stoichiometry Stoichiometry is a fancy chemistry word meaning “to calculate quantities in a chemical reaction”. Or in other words, if I mix this much of.

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Presentation transcript:

Stoichiometry Stoichiometry is a fancy chemistry word meaning “to calculate quantities in a chemical reaction”. Or in other words, if I mix this much of “X” and this much of “Y” they will react to form this much of “Z”.

Set Up of Stoich Problems In most stoichiometry problems we are using a known mass and the balanced equation coefficients to determine the mass of an unknown

Mole Ratios!!!! Keep in mind that the coefficients in the balanced equation are mole ratios, NOT mass ratios (this means you have to get things into moles first)

Steps to Solving Stoich. Problems Write and balance the chemical equation Convert the mass of the known chemical to moles (mass/molar mass) = moles Use the mole ratio to find moles of unknown chemical(s). 4. Convert moles of unknown chemical to mass moles x molar mass = mass

Caveat Just a note… A common question is – “do you include the balancing coefficient in the molar mass?” The answer is – NO! You need to use the subscripts in the molar mass, but NOT the balancing coefficients!

Example #1 A strip of zinc metal with a mass of 2.00 g is placed in an aqueous solution containing 2.50 g of silver nitrate. How many grams of silver will form? Step 1: Write and balance the chemical equation Zn (s) + 2 AgNO3 (aq)  2 Ag (s) + Zn(NO3)2 (aq)

Example #1- Step 2 A strip of zinc metal with a mass of 2.00 g is placed in an aqueous solution of silver nitrate. How many grams of silver will form? Step 2: Convert the mass of the known chemical to moles (mass/molar mass) = moles

Example #1-Step 3 Zn (s) + 2 AgNO3 (aq)  2 Ag (s) + Zn(NO3)2 (aq) Step 3: Use the coefficients of the balanced equation to determine the mole ratios.

Example #1-Step 5 Step 5: Convert moles of unknown chemical to mass moles x molar mass = mass

Example #1-Step 2 A strip of zinc metal with a mass of 2.00 g is placed in an aqueous solution containing 2.50 g of silver nitrate. How many grams of silver will form? Step 2: Convert the mass of the known chemical to moles (mass/molar mass) = moles

Example #1-Step 3 Zn (s) + 2 AgNO3 (aq)  2 Ag (s) + Zn(NO3)2 (aq) Step 3: Determine limiting reagent (limiting reagent is the reagent that doesn’t fulfill the mole ratio of the balanced equation). Use the coefficients of the balanced equation to determine the mole ratios. Limiting Reagent

Example #1-Step 4 Use the mole ratio to find moles of unknown chemical(s). You MUST use the moles of the limiting reagent to determine the moles of the unknown.

Example #1-Step 5 Step 5: Convert moles of unknown chemical to mass moles x molar mass = mass

Stoichiometry Steps Write and balance the chemical equation Convert the mass of the known chemical to moles (mass/molar mass) = moles Determine limiting reagent (limiting reagent is the reagent that doesn’t fulfill the mole ratio of the balanced equation). Use the coefficients of the balanced equation to determine the mole ratios.

Stoichiometry Use the mole ratio to find moles of unknown chemical(s). You MUST use the moles of the limiting reagent to determine the moles of the unknown. Convert moles of unknown chemical to mass moles x molar mass = mass Repeat if necessary for other chemicals Just a note… A common question is – “do you include the balancing coefficient in the molar mass?” The answer is – NO! You need to use the subscripts in the molar mass, but NOT the balancing coefficients!