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Descripción
Fichas por Maxim Korvatskyy, actualizado hace más de 1 año
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Creado por Maxim Korvatskyy
hace casi 8 años
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| Pregunta | Respuesta |
| hello | hello ∆ |
| Rate = k[C][D]^d | questions will usually be around finding K given [C] and [D] (concentrations) |
| (rate equations) k only changes as what changes? concentration? pressure? temperature? molarity? | k = Ae^(–Ea/RT) k only changes due to ∆Temperature |
| You'll be asked to use graphs to deduce order of reaction of a reagent. there are two main types: Rate/[conc.] and [conc.]/time turn over plz. | Rate/[conc.] are easy; change in conc can either cause no change in rate (0th order), linear change in rate (1st order), or quadratic change (2nd order). [conc.]/time are a bit more tricky; as time goes on, concentration will either decrease in linear fashion (0th order), bit bent (1st order) or really bent (2nd order) |
| Rate equation contains reactants which are present in (slowest) rate limiting step. (recall mechanisms and how improbable they can be) | Using [reagents] present in rate equation you can comment on whether their addition will speed up the reaction by much. |
| Each temperature has it's very own Kc,which must stay constant for the given temperature no matter what. | If you are having trouble with Kc, dedicate a day to learning it really well. Please avoid confusion at all costs. |
| what affects Kc? catalyst? amount of products? temperature? pressure? nothing? | only temperature, since each temperature value has its own dedicated Kc value. |
| Kp is used for gas systems. you can't use concentrations for gases easily, so partial pressure is used instead. what's the equation of Kp then? | Where (Pc)^c is partial pressure of (product) C to the power of mols of C. |
| Partial pressure of [A] is equivalent to fraction of total pressure which A is responsible for. {(Total pressure)x(Mol(A)/total.Mol)} | we assume that any gas (big or small) molecule exerts the same pressure as any other gas molecule in the same quantity. |
| Brønsted–Lowry theory acid is anything that gives out H+ base is anything that accepts H+ | Salt of what-used-to-be-weak-acid can act as a base and accept protons similarly, what-used-to-be-base can release the H+ and act as an acid |
| pH (Power of hydrogen [H+]x10^pH) -log[H+] = pH | water can dissociate into H+ and OH- we are only concerned about the H+ usual concentration of H+ in pure water is 0.0000001 mol/dm^3 (thats 1x10^7, which is pH=7) |
| what's the pH of the following [H+] concentrations? 0.000001 0.00001 0.001 0.1 1.0 10.0 . | 6 5 3 1 0 -1 -log(weight of the protons/their volume dm^3) |
| temprf | gssggs |
| The last peak in TOF Spectrometer of a molecule shows what? | Last M/Z number IS the total relative mass for the molecule. |
| You'll need to know the reactions of Nitrotuolene. This is mostly for organic reactions section, but it is a common conversion. | Tin metal Sn donates electrons and HCl donates protons. Reacting these with -NO2 group changes it to -NH2 group. This reaction requires 7e- and 6H+. Mechanism not required, imagine it like a porridge reacting- a mess. |
| Get to know Organic reactions, make reactants your friends, and you'll ace organic test questions. | Carbonate- test for acid (CO2) Tollens silver mirror for aldehydes |
| I hope you remember ∆H you'll need some strength if you don't. Define ∆Hf | ∆Hf - enthalpy change when 1mol of compound is made from its elements in their standard states. there are more of these... |
| ∆H -general change of energy stored in bonds ∆Hc - when 1mol of [x] is completely burnt in excess O2 ∆Hf - when 1mol of [x] is made from its elements in their standard states ∆Hat - when 1 mol standard state [x] is converted to 1mol geseous [x] ∆Hd - when 1mol worth of covalent bonds is broken | ∆Hi - when 1mol of e- is made from 1mol of gaseous [x] ∆Hea - when 1mol gaseous [x] becomes 1mol gaseous [x]1- (by absorbing electrons) ∆Hl (formation) - when 1mol of ion lattice is made from its charged gaseous components. ∆Hhyd - 1mol of gaseous [x] is completely hydrated by water (link to metal complex ions) ∆Hsol - 1mol of solid dissolved completely in water |
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