Equilibrium Test
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Created by:
kawaiihime on April 19, 2010
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43 terms
Terms | Definitions |
|---|---|
 Phase Equilibrium | Freezing point is an example of...? [Ex. H₂O (s) <=> H₂O (l)] |
| Solution Equilibrium | Saturation is an example of...? [Ex. NaCl (s) <=> Na⁺(aq) + Cl⁻(aq)] |
| Closed System | conditions where energy can leave, but matter can't |
| temperature and concentration | Rate of reaction depends on...? (2) |
| concentration | If temperature is constant, rate only depends on...? |
| Equilibrium Point | when the forward and reverse reaction proceed at equal rates |
| fewer; more; much; great; the forward reaction is favored | As H₂ and O₂ molecules collide, there are __ and __ reactants and __ and __ products. At some point there is so __ product and the chance of these particles colliding is so __ that even if __, the forward and reverse reaction proceed at equal rates. |
| the rate of a reaction is directly proportional to the product of the molar (M) concentration of the reaction species | Law of mass action |
| determine how fast a reaction proceeds, and to what extent the products are formed before reaching equilibrium | Constant equilibrium is used to...? |
| Keq = [C]c [D]d / [A]a [B]b | General rule at constant temperature for Keq when aA + bB <=> cC + dD |
| In theory, yes, but in reality, no. | Are all reactions reversible? |
| there are more products and less reactants; forward reaction is favored | Keq > 1 (2) |
| there are more reactants and less products; reverse reaction is favored | Keq < 1 (2) |
| when a system at equilibrium is subjected to as stress, the equilibrium will shift in the direction that tends to counteract the effect of the stress | LeChatelier's Principle |
| favors forward reaction; shifts to the right | If increase in formation of products, which reaction is favored? which way does the equilibrium shift? |
| favors reverse reaction; shifts to the left | If increase in formation of reactants, which reaction is favored? which way does the equilibrium shift? |
| concentration, temperature, pressure | What stresses cause a change in equilibrium? |
| right; more A will react with B which then forms more products C + D; decreases; increase | A + B <=> C + D If increase [A], the reaction will shift to the __ because __. What happens to [B]? to [C] and [D]? (2) |
| left; an increase in A is wanted; increases; decrease; does not change | A + B <=> C + D If decrease [A], the reaction will shift to the __ because __. What happens to [B]? to [C] and [D]? to the Keq? |
| temperature | only stress where the Keq will change |
| left; endothermic; increase temperature is relieved by absorbing heat; increase; decrease; decrease | A + B <=> C+ D + heat If increase temperature, the reaction will shift to the __. The __ reaction is favored because __. What happen to [A] and [B]? to [C] and [D]? to the Keq? |
| right; exothermic; decrease temperature is relieved by giving off heat; decrease; increase; increase | A + B <=> C+ D + heat If decrease temperature, the reaction will shift to the __. The __ reaction is favored because __. What happen to [A] and [B]? to [C] and [D]? to the Keq? |
| change in concentration balances out the volume change caused by pressure; fewer; more | Why is does pressure not change the Keq of a substance? Increase pressure favors __ molecules. Decrease pressure favors __ molecules. |
| right; left | N₂(g) + 3H₂(g) <=> 2 NH₃(g) If pressure increases, equilibrium will shift to the __. If pressure decreases, equilibrium will shift to the __. |
| make ammonia; N₂(g) + 3H₂(g) <=> 2 NH₃(g) + 22kj | The Haber process was used to...? Give the chemical reaction. |
| endothermic (reverse); high; increase the rate of both reactions | N₂(g) + 3H₂(g) <=> 2 NH₃(g) + 22kj Although increase temperature favors the __ reaction, the Haber process needed __ temperature to __ so that equilibrium is arrived at faster. |
| high; increased; forward; fewer | N₂(g) + 3H₂(g) <=> 2 NH₃(g) The Haber process needed __ pressure because __ pressure would favor the __ reaction with __ molecules. |
| by drawing off NH₃ while adding more H₂ and N₂; not | N₂(g) + 3H₂(g) <=> 2 NH₃(g) How did the Haber process manipulate concentrations to favor the formation of Ammonia? The reaction is __ allowed to reach equilibrium. |
| equilibrium is arrived at faster; Platinum (Pt); Iron (Fe); no | In the Haber process, catalysts are used so that __. Do catalysts such as __ or __ cause a shift in equilibrium? |
| dilute; greater 1; 0.1 and 1; less; 0.1 | Solution can be either concentrated or __? "Soluble" is __ than __g/100g H₂O. "Slightly soluble" is between __-__g/100g H₂O. "Insoluble" is __ than __g/100g H₂O |
| solubility product constant; to predict concentration | What is Ksp? What is Ksp used for? |
| the molar concentration of a liquid or solid is constant | AB <=> A⁺+ B⁻ When solving for Ksp, why can the dividing by the reactant concentration be eliminated from the equation? |
| Ksp = the product of the molar concentrations of the ions each raised to the appropriate power | Ksp equation |
| soluble; insoluble | Compounds with higher Ksp tend to be more __. Compounds with lower Ksp tend to be more __. |
| the number of moles of solute that are dissolved in a saturated solution per liter | molar solubility |
| Increase S⁻² ions; left; even less | PbS(s) <=> Pb⁺²(aq) + S⁻²(aq) What happens if very soluble Na₂S(s) is added into the aqueous solution of relatively insoluble PbS(s)? This causes a shift to the __ in the first reaction and therefore __ PbS remains in solution. |
| Ksp; state chart; reactants; Ksp; will; Ksp; will not | To determine whether a compound will precipitate out of solution: Look up the __ of the compound in your __. Using the information given in the problem, calculate the molar concentration of the __ and find the __. If the __ you found is greater than the official __ then the compound __ precipitate out. If the __ you found is less than the official __, the compound __ precipitate out. |
| divided by two | When determining whether a compound, such as AgCl, will precipitate out of solution: If 1L of of 1x10⁻³M AgNO₃ is mixed with 1L of 1x10⁻²M of NaCl, you must __ because now the reactant concentrations are moles per 2L. |
| [x]; [2x]; Ksp = [x][2x]²= 4x³ | When solving for the Ksp remember to check the coefficients of the reactants: [Ex. AB₂ <=> A + 2B] If we let the concentration of AB₂ to be [x], then what are [A]? and [B]? How is the Ksp equation written? |
| fewer collisions | Why does an increase in the pressure of a gas-phase equilibrium favor the formation of fewer molecules of gas? |
| no change | Given N₂(g) + O₂(g) <=> 2NO(g): What will happen if pressure is increased? decreased? |
| a chemical change in which the reactants can be re-formed from the products | reversible reaction |
| the forward and reverse reactions continue to take place even though equilibrium has been reached | Why is a chemical equilibrium described as dynamic? |
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