Term
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Definition
| Moles of Solute/Volume of solution |
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Term
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Definition
| refers to a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment. |
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Term
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Definition
1(a). Divide the mass (in grams) of the reactant by its molecular weight (in g/mol) OR
1(b). Multiply the amount used (in mL) by its density, then divide by its molar mass
2. Multiply the mass (your answer from steps 1(a) or 1(b)) by the number of moles of the reactant used in the reaction. |
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Term
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Definition
this is how much product will be synthesized in ideal conditions.
To determine this, multiply the amount of moles of the limiting reagent by the ratio of the limiting reagent and the synthesized product and by the molecular weight of the product. |
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Term
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Definition
this is how much product was actually synthesized in the experiment.
Example: 0.135 g acetylsalicylic acid |
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Term
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Definition
is the ratio between the actual yield and the theoretical yield multiplied by 100%. It indicates the percent of theoretical yield that was obtained from the final product in an experiment.
can be calculated using the mass of the actual product obtained and the theoretical mass of the product calculated using the balanced equation of the reaction. |
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Term
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Definition
| Mass of Actual Yield x 100% Mass of Theoretical Yield |
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