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43 Cards in this Set
- Front
- Back
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G is a value called .... |
Gibbs Free Energy |
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ΔG tells us whether a reaction is _____ or not.
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spontaneous |
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If ΔG is a negative number, then the reaction is _____. |
spontaneous |
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If a reaction is spontaneous, then it is called an ____ reaction. |
exergonic |
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If ΔG is a positive number, then the reaction is ____, and thus not spontaneous. |
endergonic |
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Entropy is a measure of _____ and is represented by the letter ___. |
disorder S |
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If a reaction proceeds towards more disorder, then the sign for S is _____. |
Positive |
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Reactions that move both forward and backwards have ____in the equations. |
forward and backwards arrows |
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If a reaction releases heat, then we say it is ______ and the sign for this enthalpy is ____. |
exothermic -ΔH (negative) |
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If a reaction absorbs energy, then we say it is _____ and it has a ____ sign for its enthalpy value |
endothermic positive |
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Because ΔG = ΔH - TΔS, then ΔG is largely dependent on ___________. |
temperature |
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ΔG can be calculated 2 ways, which are: 1) Using reference tables and doing _____ - _____. 2) Using ΔH, T, & ΔS in the formula, __________. |
1) "Products - Reactants" 2) ΔG = ΔH - TΔS |
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Melting of ice is an ____-thermic process and leads to ____ entropy, and if the temperature is high enough it is _____-gonic |
endo- more exer- |
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Freezing of water is an _____-thermic process and leads to ____ entropy, and if the temperature is low enough it is _____-gonic. |
exo- less exer- |
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Reference table values for ΔG and ΔH typically have unit ____/mol, whereas, ΔS is in ____/mol. |
kJ J |
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Hydrogen burns in the presence of oxygen to produce water. This reaction has a ____ value for entropy and it is ____-thermic and ____-gonic. |
negative exo- exer- |
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How can you tell that this reaction has an increase in entropy? |
There more moles on the product side than their are on the reactant side. |
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The Equilibrium Constant that is determined by using concentrations, in molarity, is.... |
Kc (K sub c) |
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The Equilibrium Constant that is determined by using gas pressure, is .... |
Kp (K sub p) |
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The equilibrium constant can be calculated by dividing the _________ by the __________. |
multiplied products raised to their coefficient powers multiplied reactants raised to their coefficient powers |
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Q is called the ___ _____ and is calculated just like Kc or Kp but is not always at equilibrium. |
reaction quotient |
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If the value for Q < K, then the reaction will shift which way? |
to the right, producing more products |
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If Q = K, then the reaction will shift which way? |
neither; it's at equilibrium |
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If Q > K, the the reaction will shift which way? |
to the left, producing reactants |
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The concept of a reaction shifting the right or left to re-establish equilibrium is called ____ principle. |
LeChatelier's |
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If a reaction is endothermic, then adding heat to the reaction will cause it to shift which way? |
to the right, favoring products |
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If a reaction is exothermic, then heat or energy is treated like a _____. Heat added to such a reaction will cause it to shift which way? |
product to the left, favoring reactants |
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if a reaction is exothermic, then cooling the reaction will cause the reaction to shift which way? |
to the right, favoring products |
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If the reactant side of a reaction has 5 moles of gases and product side has 3 moles of gases, then which way will the reaction shift if pressure is increased? |
to the right; the side with the fewer number of moles of gas; |
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If you are told that a reaction has a ΔH of -75 kJ, then cooling the reaction will cause the reaction to shift which way? |
to the right |
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A large Ka value (>1) means that .... |
the acid ionizes into H+ ions and A- ions well, favoring the products |
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A small Kb value (<1) means that the bases "BOH"..... |
does not ionize into B+ ions and OH- ions well, favoring formation of the reactants
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___, ____, & solvents are not written in equilibrium expressions. |
pure liquids (l) and solids (s) |
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A large Ksp value for a solid means that.... |
the solid dissolves well, favoring the formation of products |
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better |
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The Kw constant is called the ___ ____ constant for water and has a value of ____. |
Ion product |
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Kw is calculated by multiplying ___ x ____ . It does not include _____ in the denominator since pure ___ are not included in expressions. |
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Under non-standard conditions, Kw can be a different number. If it is, then to get the hydrogen & hydroxide concentrations, merely take the ___ ____ of Kw. |
square root (This works since Kw = the product of H & OH, which are equal. ) |
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We don't ordinarily use the p____ scale for indicating how acidic or basic something is. |
OH |
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If pH = 2, then pOH = ____ |
12 |
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If pH = 3, then the hydrogen ion concentration is ____ and the hydroxide concentration is ____. |
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If pOH = 4, then the hydroxide ion concentration is ____ and the hydrogen ion concentration is ____ and the pH is ___ |
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