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| 11852767526 | Equilibrium constant | k=products-reactants | 0 | |
| 11852767527 | K>1 | Forward reaction is favored | 1 | |
| 11852767528 | Forward reaction | Reactants to Products | 2 | |
| 11852767529 | Reverse reaction | Products to reactants | 3 | |
| 11852767530 | K<1 | Reverse reaction is favored | 4 | |
| 11852767531 | K=1 | neither reaction is favored | 5 | |
| 11852767532 | Small equilibrium constant means... | reactants are favored | 6 | |
| 11852767533 | Large equilibrium constant means... | products are favored | 7 | |
| 11852767534 | Kc and Kp have what units? | they both have no units, but Kp is calculated using atm and Kc is calculated using molarity | 8 | |
| 11852767535 | 1 atm | 760 mmHg and 760 Torr | 9 | |
| 11852767536 | What equation connects Kp and Kc? | Kp = Kc(RT)deltaN [delta N= (c+d) - (a+b)] | 10 | |
| 11852767537 | Solids and liquids are... | completely omitted from calculations | 11 | |
| 11852767538 | Reaction Quotient | measures the progress of a reaction relative to equilibrium | 12 | |
| 11852767539 | How is q calculated? | Same way as Kc | 13 | |
| 11852767540 | Difference between K and Q | Q depends on what STATE of the reaction and K has a given temperature that has only one value that specifies a relative amount | 14 | |
| 11852767541 | If the reaction only contains reactants... | Q = 0 | 15 | |
| 11852767542 | If the reaction only contains products... | Q = infinity | 16 | |
| 11852767543 | At equilibrium.... | K = Q | 17 | |
| 11852767544 | Q > K | reactions goes to the left (reactants) | 18 | |
| 11852767545 | Q < K | reaction goes to the right (products) | 19 | |
| 11852767546 | Q = K | reaction is at equilibrium | 20 | |
| 11852767547 | Solubility product constant (Ksp) | Measures solubility of a compound |  | 21 |
| 11852767548 | Molar solubility | Solubility of a compound in. moles per liter | 22 | |
| 11852767549 | Gibbs free energy equation with K | Grxn = -RT lnK At equilibrium G = 0 | 23 | |
| 11852767550 | When K<1 and Q=1 | lnK is negative, G is positive, the reaction is spontaneous in the reverse direction | 24 | |
| 11852767551 | When K>1 and Q=1 | lnK is positive, G is negative, the reaction is spontaneous in the forward direction | 25 | |
| 11852767552 | Le Chateller's Principle | when a chemical system at equilibrium is disturbed, the system shifts in the direction that minimizes the disturbance | 26 | |
| 11852767553 | Adding product... | shifts left | 27 | |
| 11852767554 | Adding reactant... | shifts right | 28 | |
| 11852767555 | Removing product... | shifts right | 29 | |
| 11852767556 | Removing reactant... | shifts left | 30 | |
| 11852767557 | Increasing volume... | decrease in pressure and shifts toward the side with the more moles | 31 | |
| 11852767558 | Decreasing volume... | increase in pressure and shifts toward the side with the least amount of moles | 32 | |
| 11852767559 | In an endothermic reaction, increasing temperature means... | adding reactant, shifts right, and the value of K increases because the concentration of the products increase and the concentration of the reactants decrease. | 33 | |
| 11852767560 | In an endothermic reaction, decreasing temperature means... | removing reactant, shifts left, value of K decreases because the concentration of the products decrease and the concentration of the reactants increase. | 34 | |
| 11852767561 | In an exothermic reaction, increasing temperature means... | adding product, shifts left, value of K decreases because concentration of the products decrease and the concentration of the reactants increase. | 35 | |
| 11852767562 | In a exothermic reaction, decreasing temperature means... | removing product, shifts right, value of K increases because the concentration of the products increase and the concentration of the reactants decrease. | 36 | |
| 11852767563 | Adding a catalyst... | DOES NOT change the concentration | 37 | |
| 11852767564 | Adding an inert gas... | DOES NOT change the concentration | 38 | |
| 11852767565 | If the reaction is reversed | invert Kc | 39 | |
| 11852767566 | If the reaction is multiplied | raise Kc to the power | 40 | |
| 11852767567 | If the reaction is added | multiply Kc | 41 |
