Have this confounding set of datas which I have had a hard time analysing
2ClO2 (aq) + 2OH- (aq) -> ClO3- (aq) + ClO2 - (aq) + H2O (l)
6 expts were carried out with differing concentrations of ClO2 and OH- in each expt.
The measurement of how quickly Cl)2 disappears is given in the table for each of the 6 expts. How quickly a reactant disapppears is a good measurement of how fast a reaction takes place
Concentraion of ClO2 Conc. of OH- Intial rate of disappearance
0.02 0.03 0.00276
0.04 0.03 0.01104
0.02 0.06 0.00552
0.04 0.06 0.02208
0.04 0.09 0.03312
0.120 0.030 0.09936
What is the relationship betweeen the concentrations of the reactants and the rate of reaction? Explain answer using results in the table, stating clearly the experimental data used.
This is weird. Rate of reaction doesnt increase with concentration so I can't really describe. Some of the comparison shows that concentraion increase will increase speed of reaction but most doesn't
Do take a close look at the data Many thanks
1st order w.r.t hydroxide ions
2nd order w.r.t. chlorine dioxide
3rd order reaction overall
Notice that comparing the 1st and last experiment, when you increase the molarity of chlorine dioxide 6 times, whilst keeping the molarity of hydroxide ions constant, the rate of reaction increases 6^2 = 36 times.
Originally posted by UltimaOnline:1st order w.r.t hydroxide ions
2nd order w.r.t. chlorine dioxide
3rd order reaction overall
Notice that comparing the 1st and last experiment, when you increase the molarity of chlorine dioxide 6 times, whilst keeping the molarity of hydroxide ions constant, the rate of reaction increases 6^2 = 36 times.
Hallo
thanks!
Hi regarding the ealier question heres my explanation. Could someone please help me take a look?
As the concentration of reactants increases, initial rate of disappearance of ClO3 increases, resulting in a faster rate of reaction . Using data set from expt 1 and 6 where the concentration of OH- remains the same and expt 6 has higher cntrcn of ClO2(0.120mol./dn3) while expt 1 only has 0.020mol/dm3 of ClO2, we notice that intial rate of disappearance of ClO2 in expt 6 is faster. By increasing molarity of ClO2 by 6 times, the initial rate of disappearance of ClO2 increases by 36 times. In expt 1 rate of disppearance of ClO2 is 0.00276mol/dm3/s while that in 6 is 0.09936mol/dm3/s. On the other hand, increaing cntrn of OH - will also result in faster rate of disappeance of ClO2. Using data set 1 and 3 where cntrn of ClO2 is the same in both cases at 0.02mol/.dm3 and expt 1 has lower contrn of OH 0 (0.030mol/dm3) than expt 3, at 0.06mol/dm3. Again rate of disappearance of ClO2 for expt 3 at 0.00552mol/dm3/s is faster than 0.00276mol/dm3/s for expt 1
I think I am too long winded and my key points are not well written. Where did I go wrong in any way?
Later on theres this question
Does the reaction rate depend on the contrntion of ClO2 and OH- equally? Explain your answer using results from the table. State which experimental data you are using and show clearly how you arrived at your answer.
I think its yes and in fact the above explanation i gave seems more appropriate for this question. Comment on my answer and please modify wherever necessary Thanks people!