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Chem 202 Test 2
| Question | Answer |
|---|---|
| -E cell (harder or easier to remove e-) | harder to remove an electron than H More likely to be oxidized |
| +E cell (harder or easier to remove e-) | easier to remove electron than H More likely to be reduced |
| Nernst Equation | Ecell= Ecell - 0.059/n x log (products/reactants) |
| Faraday constant | 9.64846 x 10^4 |
| - Delta G (spontaneous or non) | spontaneous |
| Delta G = -n F Ecell (kJ/mmol or J/mol) | J/mol |
| R= | 8.3145 |
| -RTlnK=-nFEcell | Ecell= RTlnK/nF |
| k (0 order) | mol/Lxs |
| k (1 order) | 1/s |
| k (2 order) | L/molxs |
| k (3 order) | L2/mol2xs |
| 1st order (integrated rate law) | ln [a] = -kt + ln [a0] |
| half life- first order | t1/2= ln2/k |
| 2nd order (integrated rate law) | 1/[a] = kt + 1/[a0] |
| half life- second order | t1/2= 1/k[a] |
| zero order (integrated rate law) | [a] = -kt + [a0] |
| half life- zero order | t1/2= [a]/2k |
| k (positive/negative slope) - 1st order | negative slope |
| k (poisitve negative slope) - 2nd order | positive slope |
| k (positive negative slope) - 0 order | negative slope |
| Focus on large or small concentrations? | small |
| rate determining step | first slow reaction |
| Arrhenius Equation | lnk = - (Ea/R) (1/T) + ln[A] |
| m (Arrhenius Equation) = | -Ea/R |
| Two Point Form | ln(k2/k1) = -Ea/R (1/T2-1/T1) |
| If atomic number matches the element but the mass # is higher | Beta Emission |
| When is neutrino a product | Beta Emission and electron capture |
| If atomic # matches element but the mass # is lower | Positron emission |
| When is an antineutrino released | In positron emission |
| if atom has correct # of protons and same mass as the periodic table | electron capture (gamma) |
| when above Bismuth | alpha-decay |
| Kinetics is always what order | first |
| Rate law of kinetics | N= Ni e^-kt or lnN = -kt + ln Ni |
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