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- 1. Mr Field
- 2. INTRODUCTION ο§ The purpose of this presentation, is to collect all the calculations you need for IB Chemistry in one place. ο§ This will help you to memorise them. ο§ It will not help you to master themβ¦the only shortcut to mastery is many hours of dedicated practice. ο§ Good luck!
- 3. PURPOSE: CALCULATING A QUANTITY IN MOLES FROM A NUMBER OF PARTICLES The Calculation Notes π π= πΏ n = the quantity in moles N = the number of particles L = Avogadroβs constant, 6.02x1023 ο§ When calculating numbers of atoms within molecules, multiply the number of particles (N) by the number of atoms in the formula ο§ To find out numbers of particles, rearrange to: N = n.L STOICHIOMETRY
- 4. PURPOSE: DETERMINE RELATIVE MOLECULAR OR FORMULA MASS, MR The Calculation ππ = (ππ’ππππ ππ ππ‘πππ . ππ‘ππππ πππ π ) Notes ο§ Mr has no unit as it is a relative value ο§ To calculate molar mass, Mm, just stick a βgβ for grams on the end STOICHIOMETRY
- 5. PURPOSE: CALCULATE A QUANTITY IN MOLES, FROM A MASS OF A SUBSTANCE The Calculation Notes π π= ππ n = the quantity in moles m = the mass of substance you are given in grams Mm = the molar mass of the substance ο§ To determine the mass of a given number of moles of a substance use: ο§ π= π π. π ο§ To determine the molar mass of a given mass of a substance: π ο§ ππ= π STOICHIOMETRY
- 6. PURPOSE: DETERMINE EMPIRICAL FORMULA FROM % COMPOSITION BY MASS The Calculation 1. Divide each % by the atomic mass 2. Divide each answer to Step 1 by the smallest answer to Step 1 3. Notes ο§ You can follow the same method if you Multiply all answers to Step 1 to remove any obvious fractions have plain composition by mass rather than % composition by mass. a. If there is a β.5β multiply everything by 2 b. If there is a β.33β multiply everything by 3 etc STOICHIOMETRY
- 7. PURPOSE: DETERMINE MOLECULAR FORMULA FROM EMPIRICAL FORMULA The Calculation ππ πΉπ = . πΉ π(πΉπ ) π Notes ο§ This and the previous calculation are often combined together in exam questions Fm = molecular formula Mr = relative molecular mass Fe = empirical formula m(Fe) = empirical formula mass STOICHIOMETRY
- 8. PURPOSE: USE MOLE RATIOS TO DETERMINE THE NUMBER OF MOLES OF βBβ THAT CAN BE MADE FROM βAβ The Calculation ππ’ππππ ππ π΅ ππ πππ’ππ‘πππ π π΅ = π π΄ . ππ’ππππ ππ π΄ ππ πππ’ππ‘πππ Notes ο§ The second term in this equation is the mole ratio ο§ You must use a fully balanced equation ο§ This is the central step in many stoichiometry calculations STOICHIOMETRY
- 9. PURPOSE: CALCULATE THEORETICAL YIELD The Calculation Notes ο§ Use mole ratios to determine the ο§ n/a expected quantity of product in moles ο§ Use π = π π . π to determine the expected mass. STOICHIOMETRY
- 10. PURPOSE: DETERMINE LIMITING AND EXCESS REACTANTS The Calculation Notes ο§ Divide moles of each reactant by their ο§ You would often then need to use mole coefficient in the balanced equation ο§ Smallest value ο limiting ratios to determine a quantity of product (in moles). ο§ Largest value ο excess STOICHIOMETRY
- 11. PURPOSE: CALCULATING PERCENTAGE YIELD. The Calculation πππ‘π’ππ π¦ππππ % πππππ = . 100 π‘βπππππ‘ππππ π¦ππππ Notes ο§ Actual and theoretical yield must have the same units. ο§ You might sometimes be required to rearrange this equation, or use it to work backwards from this to find the amount of reactant you started with. STOICHIOMETRY
- 12. PURPOSE: APPLY AVOGADROβS LAW TO CALCULATE REACTING VOLUMES OF GASES The Calculation Notes π1 π2 = π1 π2 V1 = the initial volume of gas n1 = the initial quantity of gas in moles V2 = the final volume of gas n2 = the final volume of gas in moles ο§ Only applies when temperature and pressure remain constant. ο§ Units of V do not matter. But must be the same. ο§ This is really a special case of the Ideal Gas Law where the pressure, temperature and gas constant terms cancel each other out. STOICHIOMETRY
- 13. PURPOSE: CALCULATE MOLAR QUANTITIES OF GASES AT STANDARD TEMPERATURE AND PRESSURE The Calculation Notes π π= 22.4 ο§ Only applies at standard conditions: ο§ 273 K (0oC) ο§ 101,000 Pa (1.00 atm) n = quantity in moles V = the volume of gas in dm3 22.4 is the molar volume of an ideal gas at 273K and 101,000 Pa ο§ If volume of gas is given in m3, use 2.24x10-5 as your molar volume. ο§ Molar volumes are given in the data booklet and do not need memorising. STOICHIOMETRY
- 14. PURPOSE: THE IDEAL GAS EQUATION The Calculation ππ = ππ π Notes ο§ In practice, you can often use: ο§ V in units of dm3 P = pressure in Pa V = volume of gas in m3 n = quantity of gas in moles R = the gas constant, 8.31 T = temperature in Kelvin (OC + 273) ο§ Pa in units of kPa ο§ You will need to be comfortable rearranging this equation to change the subject. ο§ This takes time to use, so only use it in non-standard conditions, or when the laws in Calculation 13 would not be quicker. STOICHIOMETRY
- 15. PURPOSE: RELATIONSHIP BETWEEN TEMPERATURE, PRESSURE AND VOLUME The Calculation Charlesβ Law, at fixed pressure: Notes π1 π1 π2 π2 = Gay-Lussacβs Law, at fixed volume: π1 π1 = ο§ These only work where the quantity in π2 π2 Boyleβs Law, at fixed temperature: π1 π1 = π2 π2 moles remains fixed. ο§ All of these are just special cases of the ideal gas law, where the remaining terms just cancel each other out. V1 and V2 are initial and final volume P1 and P2 are initial and final pressure T1 and T2 are initial and final temperature STOICHIOMETRY
- 16. PURPOSE: MOLAR CONCENTRATION The Calculation Notes π π= π c = concentration in mol ο§ Units are pronounced βmoles per decimetre cubedβ dm-3 ο§ You need to be able to use any rearrangement of this equation n = the quantity in moles V = the volume in dm3 (litres) STOICHIOMETRY
- 17. PURPOSE: CONCENTRATION BY MASS The Calculation Notes π π= π c = concentration in g dm-3 m = the quantity in grams V = the volume in dm3 (litres) ο§ Units are pronounced βgrams per decimetre cubedβ ο§ You need to be able to use any rearrangement of this equation ο§ Generally, if you have a concentration like this, you should convert it into a molar concentration before proceeding. STOICHIOMETRY
- 18. PURPOSE: DETERMINE RELATIVE ATOMIC MASS FROM % ABUNDANCE DATA The Calculation π΄π = % πππ’ππππππ (ππ‘ππππ πππ π . ) 100 Notes ο§ % abundance may be given in the question, or you may need to read it from a mass spectrum ο§ If you convert the percentages to Ar = relative atomic mass decimals (i.e. 0.8 for 80%, 0.25 for 25%), there is no need to divide by 100. ATOMIC STRUCTURE
- 19. PURPOSE: DETERMINE % ABUNDANCE FROM RELATIVE ATOMIC MASS The Calculation Notes If there are two isotopes, label one of them βaβ and one βbβ. Now: π΄ π = ο§ Ar, Ia and Ib will be provided in the question, so you can plug the numbers in, and then rearrange to find x. π₯πΌ π +π¦πΌ π π₯+π¦ However, since x+y = 100%, y = 100-x so: π΄π = π₯πΌ π +(100βπ₯)πΌ π 100 Ar = relative atomic mass Ia = the mass of isotope a Ib = the abundance of isotope b x and y is the abundance of each isotope ο§ To find y, simply do y=100-x ο§ If you have three isotopes, you must know the abundance of at least one in order to find the other two. You would also need to subtract the abundance of this one from the 100, before doing the rest of the sum. ATOMIC STRUCTURE
- 20. PURPOSE: CALCULATING THE HEAT CHANGE OF A PURE SUBSTANCE The Calculation π = ππβπ Notes ο§ Be careful of the units of massβ¦you may need to convert kg into g q = the heat change in Joules m = the mass of substance in grams ο§ Be careful of the units for specific heat capacity, if it is J K-1 kg-1 you will need to convert your mass into kg. c = specific heat capacity in J K-1 g-1 βT = temperature rise in K or OC ENERGETICS
- 21. PURPOSE: CALCULATING AN ENTHALPY CHANGE FROM EXPERIMENTAL DATA The Calculation βπ» = βππβπ βH = the enthalpy change in Joules m = the mass of solution in grams c = specific heat capacity of water: 4.18 J K-1 g-1 βT = temperature rise in K or OC Notes ο§ The minus sign is needed to ensure that an exothermic reaction has a negative enthalpy change. ο§ Units are J or kJ mol-1 ο§ The mass of solution is assumed to be the same as its volume in cm3. ο§ The specific heat capacity of the reactants is ignored. ENERGETICS
- 22. PURPOSE: CALCULATING βHR USING A HESS CYCLE The Calculation Notes Once you have produced you Hess cycle: ο§ See the βEnergeticsβ PowerPoint for 1. Write the relevant βH onto each arrow 2. Multiply each βH in accordance with the stoichiometry 3. advice on constructing Hess cycles. To do your sum, add when you go with an arrow, and subtract when you go against one. ENERGETICS
- 23. PURPOSE: CALCULATING βHR FROM AVERAGE BOND ENTHALPIES The Calculation Notes Method 1: Make a Hess cycle, then do as in Calculation 20. ο§ It is more reliable to use Hess cycles Method 2: βπ» π ο§ Average bond enthalpies can be found = πππππ‘πππ‘ πππππ β and you can easily forget whether it is reactants β products or vice versa. in Table 10 of the data booklet. (πππππ’ππ‘ πππππ ) ο§ You only need to worry about the bonds that broken and made. If a bond, for example a C-H is present at the start and finish, you can ignore itβ¦.this can save time in exams. ENERGETICS
- 24. PURPOSE: CALCULATING βHR FROM ENTHALPIES OF FORMATION The Calculation Notes Method 1: Make a Hess cycle, then do as in Calculation 20. ο§ It is more reliable to use Hess cycles Method 2: βπ» π ο§ βHof for elements in their standard = βπ» ππ (πππππ’ππ‘π ) β and you can easily forget whether it is products β reactants or vice versa. states is zero. βπ» ππ (πππππ‘πππ‘π ) βHr = enthalpy change of reaction βHof = enthalpy change of formation ο§ βHof values for many compounds can be found in Table 11 of the data booklet. ο§ In some questions, you may also need to take a state change into account, if standard states are not used. ENERGETICS
- 25. PURPOSE: CALCULATING βHR FROM ENTHALPIES OF COMBUSTION The Calculation Notes Method 1: Make a Hess cycle, then do as in Calculation 20. ο§ It is more reliable to use Hess cycles Method 2: βπ» π ο§ βHoc for CO2 and H2O is zero. = βπ» ππ (πππππ‘πππ‘π ) β βπ» ππ (πππππ’ππ‘π ) and you can easily forget whether it is reactants β products or vice versa. ο§ βHoc values for many compounds can be found in Table 12 of the data booklet. βHr = enthalpy change of reaction βHoc = enthalpy change of combustion ENERGETICS
- 26. PURPOSE: CALCULATING LATTICE ENTHALPY The Calculation Notes You need to build a Born-Haber cycleβ¦.see the Energetics PowerPoint for help. ο§ n/a ENERGETICS
- 27. PURPOSE: CALCULATING βS FROM STANDARD ENTROPY VALUES The Calculation βπ π = π π (πππππ’ππ‘π ) β Notes π π (πππππ’ππ‘π ) ο§ Units are J K-1 mol-1 ο§ So values can be found in Table 11 of the data booklet βSo = standard entropy change of reaction ο§ You cannot assume that So of an element is zero. It is not. So = standard entropy of each substance ENERGETICS
- 28. PURPOSE: CALCULATING βGR STANDARD GIBBβS FREE ENERGY OF FORMATION VALUES The Calculation Notes Method 1: Make a Hess cycle, then do similar to Calculation 20. ο§ Units are J or kJ mol-1 ο§ It is more reliable to use Hess cycles and you can easily forget whether it is products β reactants or vice versa. Method 2: βπΊ π = βπΊ ππ (πππππ’ππ‘π ) β βπΊ ππ (πππππ‘πππ‘π ) βGr = Gibbβs free energy of reaction βGof = Gibbβs free energy of formation ο§ βGof for elements in their standard states is zero. ο§ βGof values for many compounds can be found in Table 11 of the data booklet. ENERGETICS
- 29. PURPOSE: CALCULATING βGR FROM EXPERIMENTAL DATA The Calculation βπΊ = βπ» β πβπ βG = Gibbβs free energy βH = Enthalpy change Notes ο§ If βH is in kJ mol-1, you will need to divide βS by 1000 to convert it to units of kJ K-1 mol-1 ο§ You may first need to calculate βH and βS using Calculations 23 and 24. T = Temperature in Kelvin βS = Entropy change ENERGETICS
- 30. PURPOSE: CALCULATE THE RATE OF A REACTION The Calculation ββ[π ] β[π] π ππ‘π = = βπ‘ βπ‘ β[R] = change in reactant concentration Notes ο§ Units are mol dm-3 s-1 ο§ The minus sign in front of β[R] is because the concentration of reactants decreases β[P] = change in product concentration βt = change in time KINETICS
- 31. PURPOSE: CALCULATE THE GRADIENT OF A SLOPE The Calculation πβππππ ππ π¦ πΊπππππππ‘ = πβππππ ππ π₯ Notes ο§ Used for calculating rate from graph of concentration (y-axis) over time (xaxis) KINETICS
- 32. PURPOSE: DETERMINE THE ORDER OF REACTION WITH RESPECT TO A REACTANT, X. The Calculation 1. 2. Identify two experiments, where the concentration of βxβ has changed, but all others have remained the same. Compare the change in [x] to the change in rate: a. If doubling [x] has no effect on rate, Notes ο§ Sometimes, you canβt find two cases where only [x] has changed, in which case you may need to take into account the order of reaction with respect to other reactants. then 0th order. b. If doubling [x] doubles rate, then 1st order. 3. If doubling [x] quadruples rate, then 2nd order. KINETICS
- 33. PURPOSE: DEDUCE A RATE EXPRESSION The Calculation π ππ‘π = π[π΄] π₯ [π΅] π¦ [πΆ] π§ Notes ο§ Reactants with a reaction order of zero can be omitted from the rate equation k = rate constant (see below) [A/B/C] = concentration of each reactant x/y/z = order of reaction with respect to each reactant ο§ Given suitable information, you may need to calculate the value of the rate constant if given rates, concentrations and reaction order, or the expected rate given the other information. KINETICS
- 34. PURPOSE: DETERMINING THE UNITS FOR THE RATE CONSTANT The Calculation πππ ππβ3 π β1 ππππ‘π = πππ π₯ (ππβ3 ) π₯ ο§ mol and dm-3 terms on the top and the bottom should be cancelled out ο§ Remaining mol and dm-3 terms on the bottom should then be brought to the top by inverting their indices. Notes ο§ If you canβt understand this, try to memorise: ο§ 0th order: mol dm-3 s-1 ο§ 1st order: s-1 ο§ 2nd order: mol-1 dm3 s-1 ο§ 3rd order: mol-2 dm6 s-1 x = the overall order of the reaction KINETICS
- 35. PURPOSE: DETERMINING ACTIVATION ENERGY Notes The Calculation ο§ The Arrhenius equation: π = π΄π ο§ This rearranges to: ln π = βπΈ π 1 .π π βπΈ π π π + ln π΄ ο§ Which is basically the equation for a straight line in the form βy=mx+cβ where: βyβ is ln k; βxβ is 1/T; βmβ is βEa/R; βcβ is ln A ο§ So, if we do a reaction at a range of temperatures and calculate ln k, then: ο§ Where: ο§ ο§ ο§ ο§ ο§ ο§ k = rate constant A = Arrhenius constant e = exponential constant Ea = activation energy R = gas constant, 8.31 T = temperature in Kelvin 1. Draw a graph with 1/T along the x-axis, and ln k on the y-axis ο§ Units of Ea are kJ mol-1 2. Draw a straight line of best fit. ο§ From the graph, you might also be asked 3. Determine the gradient of the line 4. Then: πΈ π = βπΊπππππππ‘ π to calculate A: ο§ βln Aβ, is the y-intercept of the graph, so simply raise βeβ to the power of this intercept. KINETICS
- 36. PURPOSE: DETERMINING THE EQUILIBRIUM CONSTANT EXPRESSION The Calculation For the reaction: wA + zB ο yC + zD Notes ο§ Only applies to reactants for which there is a concentration: ο§ Aqueous substances are included ο§ Solids and pure liquids are omitted as they do not have a concentration per se [πΆ] π¦ [π·] π§ πΎπ = [π΄] π€ [π΅] π§ ο§ For reactions involving gases, use partial pressures instead of concentrations. ο§ At SL, you only need be able to construct the expression. Kc = equilibrium constant ο§ At HL, you may need to calculate Kc from the expression and suitable data, or to determine reactant equilibrium concentrations of reactants, given Kc and suitable information. EQUILIBRIUM
- 37. PURPOSE: DETERMINING CHANGES IN [H+] GIVEN CHANGES IN PH The Calculation Notes ο§ For each increase of β1β on the pH scale, ο§ At SL, you do not need to be able to divide [H+] by 10. ο§ For each decrease of β1β on the pH scale, calculate pH, just to understand it in relative terms. multiply [H+] by 10 ACIDS AND BASES
- 38. PURPOSE: DEDUCE [H+] AND [OH-] GIVEN KW The Calculation Notes πΎ π€ = π» + . [ππ»β ] ο§ At standard conditions, Kw = 1.00x10-14 ο§ Kw varies with temperature, so it is So: π»+ πΎπ€ = [ππ»β ] And: ππ»β important to know how to do this calculation. πΎπ€ = [π» + ] ACIDS AND BASES
- 39. PURPOSE: CALCULATING PH FROM [H+] AND VICE VERSA The Calculation Notes ππ» = βπππ10 [π» + ] [π»+ ] = 10βππ» ο§ With strong acids, you can assume [H+] is the same as the concentration of the acid (adjusted for the stoichiometry) ο§ With weak acids, you will need to calculate [H+] using Ka or pKa. ACIDS AND BASES
- 40. PURPOSE: CALCULATING PH FROM [OH-] AND VICE VERSA The Calculation Notes πππ» = βπππ10 [ππ»β ] [ππ» β ] = 10βπππ» ο§ With strong bases, you can assume [OH- ] is the same as the concentration of the acid (adjusted for the stoichiometry) ο§ With weak acids, you will need to calculate [OH-] using Kb or pKb. ACIDS AND BASES
- 41. PURPOSE: DETERMINING KA AND KB OF ACIDS/BASES AND THEIR CONJUGATE BASES/ACIDS The Calculation Notes πΎ π€ = πΎ π. πΎ π So: And: πΎπ€ πΎπ = πΎπ ο§ This is useful when trying of determine the strength the conjugate base of a weak acid, and the conjugate acid of a weak base. πΎπ€ πΎπ = πΎπ ACIDS AND BASES
- 42. PURPOSE: DETERMINING PKA AND PKB OF ACIDS/BASES AND THEIR CONJUGATE BASES/ACIDS The Calculation ππΎ π€ = ππΎ π + ππΎ π So: ππΎ π = ππΎ π€ β ππΎ π Notes ο§ This is useful when trying of determine the strength the conjugate base of a weak acid, and the conjugate acid of a weak base. And: ππΎ π = ππΎ π€ β ππΎ π ACIDS AND BASES
- 43. PURPOSE: DETERMINING PH FROM POH AND VICE VERSA The Calculation ππΎ π€ = ππΎ π + ππΎ π Notes ο§ This is useful to quickly and easily calculate one of pH/pOH from the other (or [H+]/[OH-]). So: ππ» = 14 β πππ» And: πππ» = 14 β ππ» ACIDS AND BASES
- 44. PURPOSE: CALCULATING PH OF A SOLUTION OF A WEAK ACID Notes The Calculation π»+ [π΄β ] πΎπ = [π»π΄] ο§ We assume that [HA] is equal to the concentration stated in the question, as only a very small amount has dissociated. ο§ You may need to work backwards from pH to Since [H+] = [A-]: πΎπ = π»+ 2 work out Ka: [π» + ] = 10βππ» [π»π΄] π»+ 2 So: [π» + ] = πΎ π . [π»π΄] ο§ Then: πΎ π = [π»π΄] ο§ You will not need to work out problems for Then: ππ» = βπππ10 [π» + ] polyprotic weak acids that would require quadratics. ACIDS AND BASES
- 45. PURPOSE: CALCULATING POH OF A SOLUTION OF A WEAK BASE Notes The Calculation π΅ + [ππ» β ] πΎπ = [π΅ππ»] Since [B+] = [OH-]: ππ» β 2 πΎπ = [π΅ππ»] ο§ We assume that [BOH] is equal to the concentration stated in the question, as only a very small amount has dissociated. ο§ You may need to work backwards from pOH to work out Kb: [ππ» β ] = 10βπππ» So: [ππ» β ] = Then: πΎ π . [π΅ππ»] πππ» = βπππ10 [ππ» β ] ο§ Then: ππ» β 2 πΎπ = [π΅ππ»] ACIDS AND BASES
- 46. PURPOSE: DETERMINING PH OF ACIDIC BUFFER SOLUTIONS (AND ALKALI BUFFERS) Notes The Calculation π»+ [π΄β ] πΎπ = [π»π΄] Now [H+] is not equal to [A-]: So: [π»+ ] πΎ π . [π΄β ] = [π»π΄] ο§ You may need to use your stoichiometry to calculate the [HA] and [A-] in the buffer solution first. ο§ Since additional A- is added, we now need to use the concentration of A- from the buffer as our [A-]. ο§ [HA] should either be that stated in the question, or that calculated via stoichiometry, depending on the context. ο§ For alkali buffers, do the same process Then: ππ» = βπππ10 [π»+ ] but with OH-, Kb etc. ACIDS AND BASES
- 47. PURPOSE: CALCULATE EOCELL The Calculation π πΈ ππππ = πΈ π πππ‘βπππ β πΈ π (anode) Eocell = cell potential Eo = standard electrode potential Notes ο§ The value should always be positive, so if you get it the wrong way round, just take off the minus sign. ο§ Eo can be found in the data booklet. ο§ You do not need to take the stoichiometry of the reaction into account, just use the Eoas they are in the data booklet. OXIDATION AND REDUCTION
- 48. PURPOSE: CALCULATING RELATIVE UNCERTAINTIES (IN %) The Calculation π ππππ‘ππ£π π’πππππ‘ππππ‘π¦ = Notes πππ πππ’π‘π π’πππππ‘ππππ‘π¦ .100 π ππ§π ππ π£πππ’π ο§ Large measurements have lower relative uncertainties MEASUREMENT AND PROCESSING
- 49. PURPOSE: CALCULATING ABSOLUTE UNCERTAINTY WHEN ADDITION/SUBTRACTION IS INVOLVED The Calculation Notes πππ‘ππ π’πππππ‘ππππ‘π¦ = ο§ This only works when adding and (πππ πππ’π‘π π’πππππ‘ππππ‘πππ ) subtracting values with the same units MEASUREMENT AND PROCESSING
- 50. PURPOSE: CALCULATING RELATIVE UNCERTAINTY WHEN MULTIPLICATION/DIVISION IS INVOLVED The Calculation Notes πππ‘ππ π’πππππ‘ππππ‘π¦ = ο§ For use when you are (πππππ‘ππ£π π’πππππ‘ππππ‘πππ ) multiplying/dividing values with different units MEASUREMENT AND PROCESSING
- 51. PURPOSE: CALCULATING THE ENERGY VALUE OF FOOD FROM COMBUSTION DATA The Calculation Notes Use: ο§ You may need to convert the energy π = ππβπ value into a value per mole by dividing q by the number of moles of substance burnt. q = the heat change in Joules m = the mass of substance in grams c = specific heat capacity in J K-1 g-1 βT = temperature rise in K or OC HUMAN BIOCHEMISTRY
- 52. PURPOSE: CALCULATING IODINE NUMBERS The Calculation Notes 100 ο§ π(πΌ2 ) = π πΌ2 . π(πππππ) ο§ ο§ N(I2) = the iodine number ο§ m(I2) = the mass of iodine reacting in g ο§ All units should be grams ο§ You may need to convert from data involving bromine to an βiodine equivalentββ¦just use your stoichiometry ο§ m(lipid) = the mass of lipid involved in g HUMAN BIOCHEMISTRY
- 53. PURPOSE: CALCULATE THE NUMBER OF DOUBLE BONDS IN A LIPID USING IODINE NUMBER. The Calculation Notes Calculate the quantity in moles of I2 corresponding to the iodine number: π(πΌ2 ) π(πΌ2 ) = π π (πΌ2 ) N(I2) = the iodine number Calculate the quantity in moles of lipid in 100g: 100 π(πππππ) = π π (πππππ) Then the number of double bonds is: π(πΌ2 ) π·ππ’πππ πππππ = π(πππππ) n = quantities in moles Mm = molar masses ο§ This works because each mole of double bonds reacts with one mole of iodine. HUMAN BIOCHEMISTRY

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