Term
| When calculating the enthalpy change of a reaction, does the stoichiometry of the reaction matter? |
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Definition
| Yes, it does. Enthalpy is an extensive process, so quantity does matter. |
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Term
| What is the equation for the change in enthalpy? |
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Definition
| ΔH=ΔU+PΔV and ΔH(rxn)=ΔH(products)- ΔH(reactants) |
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Term
| Removing heat from an exothermic reaction will increase or decrease the product formation? An endothermic reaction? |
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Definition
| Removing heat will push the exothermic reaction toward the products since heat is a product and is removed according to Le Chattle's principle. Removing heat from an endothermic reaction would slow the reaction and bring it toward products. |
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Term
| What is more exothermic: a phase transition or a chemical reaction? |
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Definition
| A chemical reaction will (in most all cases) be more exothermic than a phase change (eg. moving from liquid water to vapor water). |
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Term
| What is the equation for the change in gibbs free energy? |
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Definition
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Term
| The solubility product constant of mercury(I) iodide is 1.2x10^-28 at 25 degrees. Estimate the concentration of mercury ions and iodide ions in equilibrium with solid mercury(I) iodide? |
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Definition
| [I-]=6x10^-10 mol/L, [Hg22+]=3x10^-10 mol/L |
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Term
| What is the concentration of hydroxide ions in a saturated Ba(OH)2 solution? The Ksp=4x10^-3 |
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Definition
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Term
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Definition
| An ideal solution with some non-volatile solute dissolved in it will have a linear vapor pressure depression depending on the mole fraction of the solvent: P(final)=X(solvent)P(stp) |
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