a) Plot two separate graphs of rate vs concentration (lowest to highest concentration) for beakers 1-4 (graph 1) and 5-8 (graph 2). Fit a line of best fit through the data points and extrapolate the curve so that it goes through the origin (0) (see the document, Instructions for plotting graphs, for help. Graphs may be done by hand on graph paper or using Excel).

b) From both graphs, an observed rate constant, k_obs, can be determined from the slope. Calculate k_obs for both data sets using points on your line of best fit and include these values on your graphs with the correct units.

To upload your graphs for this question, attach a pdf file to the question by clicking on the page icon.

a) Plot twee afsonderlike grafieke van tempo vs konsentrasie (laagste tot hoogste konsentrasie) vir bekers 1-4 (grafiek 1) en 5-8 (grafiek 2). Pas ‘n lyn van beste passing deur die datapunte en ekstrapoleer die kurwe sodat dit deur die oorsprong gaan (0) (sien die dokument, Instruksies vir die plot van grafieke, vir hulp. Grafieke mag met die hand gedoen word op grafiekpapier of met Excel).

b) Vanaf beide grafieke kan ʼn waargenome tempokonstante, k_obs, bepaal word vanaf die helling. Bereken k_obs vir beide datastelle deur punte te gebruik op jou lyn van beste passing en gee hierdie waardes op jou grafieke met die korrekte eenhede.

Om jou grafieke op te laai vir hierdie vraag, heg 'n pdf dokument aan die vraag deur op die bladsy ikoon te kliek.

Calculate the initial concentration (1 significant figure) of KI (M) after the addition of all reagents to Beaker 5, following the procedure in your practical manual.

Bereken die aanvangskonsentrasie (1 beduidende syfer) van KI (M) nadat alle reagense, soos beskryf volgens die prosedure in jou praktiese handleiding, in Beker 5 gevoeg is.

Which concentration(s) is(are) being varied in the first part of the practical?

Watter konsentrasie(s) word in die eerste deel van hierdie praktika gevarieer?

The following data were recorded for the reaction between nitrogen dioxide (NO₂) and fluorine (F₂). What is the order of reaction with respect to nitrogen dioxide (assuming that [F₂] is constant)?

Give only the numerical value of the order, e.g. 1 (for 1st order) or 0 (for zero order).

Die volgende data is aangeteken vir die reaksie tussen stikstofdioksied (NO₂) en fluoor (F₂). Wat is die orde van die reaksie met betrekking tot die stikstofdioksied (aanvaar dat [F₂] konstant is)?

Gee slegs die numeriese waarde van die orde, bv 1 (vir 1ste orde) of 0 (vir zero orde), ens.

Consider the reaction below and use the data supplied to determine the rate law and overall order of the reaction. Write your answer for the rate law in the format e.g. k[A]6[B]3.

Oorweeg die reaksie hieronder en gebruik die data voorsien om die tempowet en algehele orde te bepaal van die reaksie. Skryf jou antwoord vir die tempowet in die formaat e.g. k[A]6[B]3.

Exp.

Eksp.

[A]

(M)

[B]

(M)

Rate/ Tempo

(M.s^-1)

Consider the reaction whereby A + B → products. The rate law was found to be rate = k[A]²[B]. If the concentration of B is doubled while the concentration of A is kept constant, with which factor will the rate of the reaction multiply (e.g. 0.25 or 0.5 or 1 or 2 or 3 or...)?

Beskou die reaksie waarvolgens A + B → produkte. Die tempowet vir hierdie reaksie is tempo = k[A]²[B]. Indien die konsentrasie van B verdubbel terwyl die konsentrasie van A konstant gehou word, met watter faktor sal die tempo van die reaksie vermenigvulding (bv. 0.25 of 0.5 of 1 of 2 of 3 of...)?

Reaction 1 (decomposition of H₂O₂ by KI) is _____ than Reaction 2 (reduction of I₂ by NaS₂O₃) and therefore there will be no _____ present in the reaction flask until all S₂O₃^2- ions have reacted.

Reaksie 1 (ontbinding van H₂O₂ deur KI) is _____ as Reaksie 2 (reduksie van I₂ deur NaS₂O₃) en daarom sal geen _____ teenwoordig wees in die reaksiefles totdat al die S₂O₃^2- ione gereageer het nie.