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| 5839516108 | Equilibrium constant | Kc = products/reactants | 0 | |
| 5839516109 | K>1 | Forward reaction is favored | 1 | |
| 5839516110 | Forward reaction | Reactants to Products | 2 | |
| 5839516111 | Reverse reaction | Products to reactants | 3 | |
| 5839516112 | K<1 | Reverse reaction is favored | 4 | |
| 5839516113 | K=1 | neither reaction is favored | 5 | |
| 5839516114 | Small equilibrium constant means... | reactants are favored | 6 | |
| 5839516115 | Large equilibrium constant means... | products are favored | 7 | |
| 5839516116 | Kc and Kp have what units? | they both have no units, but Kp is calculated using atm and Kc is calculated using molarity | 8 | |
| 5839516118 | What equation connects Kp and Kc? | Kp = Kc(RT)deltaN [delta N= (c+d) - (a+b)] | 9 | |
| 5839516119 | Solids and liquids are... | completely omitted from equilibrium expression | 10 | |
| 5839516120 | Reaction Quotient | Q = products/reactants | 11 | |
| 5839516122 | Difference between K and Q | Q uses initial quantities and K uses equilibrium quantities | 12 | |
| 5839516126 | Q > K | reactions goes to the left (reactants) | 13 | |
| 5839516127 | Q < K | reaction goes to the right (products) | 14 | |
| 5839516128 | Q = K | reaction is at equilibrium | 15 | |
| 5839516134 | Le Chateller's Principle | when a chemical system at equilibrium is disturbed, the system shifts in the direction that minimizes the disturbance | 16 | |
| 5839516135 | Adding product... | shifts left | 17 | |
| 5839516136 | Adding reactant... | shifts right | 18 | |
| 5839516137 | Removing product... | shifts right | 19 | |
| 5839516138 | Removing reactant... | shifts left | 20 | |
| 5839516139 | Increasing volume (decreasing pressure)... | shifts toward the side with the more moles | 21 | |
| 5839516140 | Decreasing volume (increasing pressure)... | shifts toward the side with the least amount of moles | 22 | |
| 5839516141 | In an endothermic reaction, increasing temperature means... | shifts right The value of K increases because the concentration of the products increase and the concentration of the reactants decrease. | 23 | |
| 5839516142 | In an endothermic reaction, decreasing temperature means... | shifts left The value of K decreases because the concentration of the products decrease and the concentration of the reactants increase. | 24 | |
| 5839516143 | In an exothermic reaction, increasing temperature means... | shifts left The value of K decreases because concentration of the products decrease and the concentration of the reactants increase. | 25 | |
| 5839516144 | In a exothermic reaction, decreasing temperature means... | shifts right The value of K increases because the concentration of the products increase and the concentration of the reactants decrease. | 26 | |
| 5839516145 | Adding a catalyst... | DOES NOT change the concentration | 27 | |
| 5839516146 | Adding an inert (Noble) gas... | DOES NOT change the concentration | 28 | |
| 5839516147 | If the reaction is reversed | invert Kc ; 1/Kc | 29 |
