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# Chem 202 Test 2

-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)
- 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
Created by: 1363731667