https://padlet.com/tfrank6302/cg46th0m1xtc By: Trinity, Eric, Alani,and Adriana en-us 2018-12-07 02:55:11 UTC 2026-01-08 19:51:30 UTC hello@padlet.com tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312105541 Stoichiometry is the calculation of reactants and products in chemical reactions. ]]> 2018-12-07 03:17:46 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312105541 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312107056 1. Theoretical yield
2. Percent yield
3. Excess reactant 
4. Limiting reactant
5. Actual yield]]> 2018-12-07 03:29:00 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312107056 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312107378 The calculated or expected amount of product is called the theoretical yield.The limiting reactant gives the smallest yield of the product calculated from the reactant available. The smallest yield of a product is called the theoretical yield. ]]> 2018-12-07 03:31:28 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312107378 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312108190 The calculated or expected amount of product is called the theoretical yield. The amount of product actually produced is called the actual yield. When you divide actual yield by theoretical yield you get a decimal percentage known as the percent yield of a reaction.]]> 2018-12-07 03:37:42 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312108190 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312109341 The excess reactant is the reactant in a chemical reaction with a greater amount than necessary to react with the limiting reactant. It is the reactant that remain after a chemical reaction has reached equilibrium.]]> 2018-12-07 03:47:16 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312109341 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312109896 The limiting reactant in a chemical reaction is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this reagent, since the reaction cannot continue without it.]]> 2018-12-07 03:51:35 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312109896 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312110314 The actual yield can be given as the weight in grams or in moles.]]> 2018-12-07 03:54:20 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312110314 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312110740 1. Convert the units of the given substance (A) to moles.
2. Use the mole ratio to calculate the moles of wanted substance (B).
3. Convert moles of the wanted substance to the desired units.

]]> 2018-12-07 03:57:26 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312110740 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312111849 2Cu + 2Ag(NO3) —> 2Ag + 2Cu(NO3)
Molar Mass Of 2Cu (Copper): 127.092g/mol
Molar Mass of 2Ag(NO3) (Silver Nitrate):
277.741g/mol
Molar Mass Of 2Ag (Silver): 215.736g/mol
Molar Mass of 2Cu(NO3): 125.551g/mol
Number of Grams For Copper: 100g
Number Grams For Silver Nitrate: 150g]]> 2018-12-07 04:06:00 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312111849 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312112598 Step 1 - “Get Moles”:
Copper - 100g Divided By 127.092g/mol = 0.787 moles
Silver Nitrate- 150g Divided By 277.741 =
0.540 moles

]]> 2018-12-07 04:11:58 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312112598 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312112788 Copper - 0.787 Multiplied By 2 Then Divided By 2 = 0.787 moles
Silver Nitrate - 0.540 Multiplied By 2 Then Divided By 2 = 0.540 moles]]> 2018-12-07 04:13:48 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312112788 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312112919 Since we already got moles we can go ahead and get the theoretical yield, percent yield excess reactant  limiting reactant, and actual yield. ]]> 2018-12-07 04:15:29 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312112919 tfrank6302 https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312115377 Copper - 0.787 (Excess)
Silver Nitrate - 0.540 (Limiting)
Theoretical: 0.540 moles x 125.551g/mol = 67.797g 2Cu(NO3)
Actual: .540 2/2 .787 —> .787 - .540 =.247 x 227.741 = 56.252g]]> 2018-12-07 04:43:11 UTC https://padlet.com/tfrank6302/cg46th0m1xtc/wish/312115377