Silver Nitrate and Calcium Chloride

Ag(NO3)+CaCl2

Type of reaction

the type of reaction is a double replacement. When doing a double replacement the positive ion and the negative ion switches places and forms a new product. The reaction given is Silver Nitrate and Calcium (Ag(NO3)+CaCl2). With this reactant you do as shown below.
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Double Reaction Example:

Ag(NO3)+CACl2 ===> Ca(NO3)+AgCl. When the reaction is done this is how it looks like.

Balancing An Equation

When balancing a equation you have to be sure that you have gotten your product. Once you have gotten your product you balance your reactant with your product. Be sure on the product side your element equals to the element on the reactant side

Before Balancing

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After Balancing

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IUPAC name for each reactant and product

Basically what this is the name of the compounds in the equation so it would go like this.


Ag(NO3)= Silver Nitrate , CaCl= Calcium Chloride. so in the equation it would look like..

Silver Nitrate+Calcium Chloride ===> Calcium Nitrate+Silver Chloride.

Molar Mass For Each Product And Reactant

When finding the molar mass of each compound you their atomic masses with each other (which is found on the P.T.) do not add the coefficents.

Molar Mass Example

Ag=107.868 So since the equation has 1 Ag, 1 N, and 3 O, you just add them up

N=14.007 107.868+14.007+3(15.999)=169.872

O=15.999 Now you do that with the other three compounds

Mole to Mole Conversion

When converting to mole to mole its just a two step problem. In the first box you put your given and then you use coefficents.

Example

If i have 11.30 moles Silver Nitrate how many moles are in Calcium Nitrate
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How the process looks and you mulitipy the top and divide by the bottom so the answer is 5.65 mol of Ca(NO3)

Mass to Mass Conversions

When doing mass to mass conversions its like mole to mole but longer steps in total there are 3 steps.
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Limiting And Excess reactant

How to find the limiting and excess reactant you have to you use the mass to mass conversions for both your givens. Once you gotten that the less product is your limiting reactant and the more product is the excess reactant.
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The first one will be your limiting reactant and the second one your excess reactant

Percent Yield

You have your actual yeild over your theoretical yield times 100

Example

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