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41 Cards in this Set
- Front
- Back
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What is energy? |
capacity to do work |
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What do we call stored energy? |
potential energy |
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Kinetic energy |
energy of motion |
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Energy can be measured in _______ or _______ |
calories, joules |
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What is a calorie? |
amount of energy needed to raise the temperature of 1 gram of water at 1 degree Celsius. |
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Delta H |
the energy absorbed or released in any reaction. (heat) |
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List 4 things that happen in an endothermic reaction: |
1. Energy is absorbed 2. H is positive 3. bonds broken in reactants are stronger than bonds formed in products 4. Products are higher in energy than reactants |
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List 4 things that happen in an exothermic reaction:
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1. Energy is released
2. H is negative 3. Bonds formed in product are stronger than bonds broken in reactants 4. Products are lower in energy than reactants |
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What is delta H? |
Energy of product - Energy of reactants |
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Energy of Activation (E^a) |
difference in energy between reactants and the transition state. It represents the minimum amount of energy that the reactants must possess for the reaction to occur. |
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When Energy Activation is high, the reactions are ______ |
slow |
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When energy activaction is low, the reactions are _____ |
fast |
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List 3 things that can affect reaction rate: |
concentration, temperature, and catalysts |
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Equilibrium |
occurs when the rate of forward reaction equals the rate of the reverse action |
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Equilibrium constant (K) = ? |
[products] / [reactants] |
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When K > 1 |
equilibrium favors the product & equilibrium lies to the right |
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When K < 1 |
equilibrium favors the reactants & equilibrium lies to the left |
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When K = 1 |
both reactants and products are present |
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Adding reactant will cause equil. to _______ |
favor the products |
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Removing reactant will cause equil. to ______ |
favor the reactants |
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Adding product will cause equil. to _____ |
favor reactants |
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Removing product will cause equil. to ______ |
favor the products |
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Increasing temp. in exothermic reaction will cause equil. to ____________ |
favor reactants |
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Increasing temp in endothermic reaction will cause equil. to _________ |
favor products |
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Decreasing temp in an endothermic reaction will cause equil. to ________ |
favor reactants |
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Decreasing temp. in an exothermic reaction will cause equil. to ____________ |
favor products |
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Increasing pressure will cause equil. to ______ |
favor side that has fewer moles |
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Decreasing pressure will cause equil. to _______ |
favor side that has more moles |
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1 calorie = _____ J |
4.184 |
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1 kcal = ______ kJ |
4.184 kJ |
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Bond breaking requires________ |
input of energy |
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Bond formation always ________ |
releases energy |
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Bond Dissociation Energy |
amount of heat in reaction for breaking a covalent bond by equally diving the electrons between 2 atoms. (always positive value) |
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the stronger the bond, the ______ its bond dissociation energy |
higher |
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When H is negative: |
more energy is released in forming bonds, & bonds formed in products are stronger |
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When H is positive: |
more energy is needed to break the bonds, & bonds broken in reactants are stronger |
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What do catalysts do? |
accelerate a reaction by lowering the Ea without effecting H |
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Bond breaking is always endothermic/exothermic? |
endothermic |
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Bond forming is always endothermic/exothermic? |
exothermic |
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3 prerequisites for an effective collison of molecules: |
1. Collision must be between the right molecules/atoms 2. Molecules must have right orientation 3. There must be enough energy present |
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Equilibrium constant (K) = |
concentration of products / concentration of reactants. (coefficients are exponents) |
