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Description
Flashcards by sofie von kaiser, updated more than 1 year ago
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Created by sofie von kaiser
about 7 years ago
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| Question | Answer |
| Error in calorimeter experiment of combustion of ethanol | not all heat produced was transferred to the water. water loses some heat to the surroundings. incomplete combustion of ethanol |
| Definie Hess's law | the enthalpy change occurs, for any reaction independent of the route, provided the initial and final conditions. |
| Defnie Standar enthalpy of formation | the enthalpy change that occurs, when one mole of substance is formed from its element in standard conditions. product-reactant |
| describe the endothermic process | breaking bonds, atoms are separated, which are attracted by electrostatic forces. Thus, needing energy. Reactants more stable than product. But enthalpy of the product is stronger. T decreases. |
| describe the exothermic process | bonds forming, so atoms are bonded together, which are attracted by electrostatic forces. Thus, releasing energy. T decreases products more stable than reactants. ENthaply of reactants greater. |
| standard enthaply of combustion | is the enthalpy change that occurs, when one mole of a substance is combusted in oxygen under standard conditions. reactants - products. |
| Emergy cycles Born haber cycle. atom and I.E | atomization: is the enthalpy change that occurs when one mole of a gaseous atom is formed from its element. I.E: is the minimum energy needed to remove one mole of gaseous electron from one mole of gaseous atom. Na+ -> Na + e- |
| Energy cycles Born Haber cycle. E.A and Lattice enthalpy | E.A: is the enthalpy change that occurs when one mole of gaseous electron is added to one mole of gaseous atom. Cl-> Cl- +e- L.E: is the enthalpy change that occurs when one mole of solid ionic compound is separated from a gaseous ion under standard conditions. |
| Predicting the Lattice Enthaply | The higher the lattice enthalpy, as the ionic radius decreases and the ionic charge increases. |
| Enthalpies change of solution | is the enthalpy change that occurs when one mole of a solute is dissolved in a solvent to infinite dilution under standard conditions. ionic compounds are soluble in water, as ions are attracted to the polar solvent water. Hsol=Hhdry + HL.E |
| define entropy (s) | refers to the distribution of available energy among particles. the higher the distribution of available energy the higher the entropy. |
| predicting entropy change values | s-> g entropy increases, as the distribution of energy is increasing, therefore the entropy is positive. |
| calculating the entropy change | s = product - reactant |
| Gibbs free energy (system) | predicts the feasibility of a reaction = H - TS |
| calculating gibbs free energy reaction | Gproduct - Greactant |
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