Back
to top
Chemistry Salters Investigation
Watch
Announcements
Page 1 of 1
Go to first unread
Skip to page:
Hi, it's a bit of a long winded one but i am trying to write up my investigation- i did the decomposition of hydrogen peroxide in the presence of inorganic transition metal catalysts. I have found the order of reaction etc and varied the temperature at which i carried out the experiment. Does anybody know how to calculate rate constant k using the arrhenius equation?
0
reply
Report
#2
Are you sure you are not mistaking something? You can use Arrhenius equation to find activation energy, once you know rate constant - but rate constant you have to find from the experimental data.
Unless you were given activation energy separately, which I doubt.
Unless you were given activation energy separately, which I doubt.
0
reply
(Original post by Borek)
Are you sure you are not mistaking something? You can use Arrhenius equation to find activation energy, once you know rate constant - but rate constant you have to find from the experimental data.
Unless you were given activation energy separately, which I doubt.
Are you sure you are not mistaking something? You can use Arrhenius equation to find activation energy, once you know rate constant - but rate constant you have to find from the experimental data.
Unless you were given activation energy separately, which I doubt.
0
reply
Report
#4
(Original post by mynameischloe)
I think i am supposed to calculate k first but am unsure how to do this from my experimental data? I then have to use k and arrhenius to calculate activation enthalpy
I think i am supposed to calculate k first but am unsure how to do this from my experimental data? I then have to use k and arrhenius to calculate activation enthalpy
0
reply
(Original post by dragonkeeper999)
I assume that you varied the concentration of each reactant in your experiments. This allows you to calculate k using the rate equation for your reaction. You can then use this value of k to calculate the activation enthalpy using the Arrhenius equation and your data from the temperature experiments
I assume that you varied the concentration of each reactant in your experiments. This allows you to calculate k using the rate equation for your reaction. You can then use this value of k to calculate the activation enthalpy using the Arrhenius equation and your data from the temperature experiments
0
reply
(Original post by Borek)
What kind of data have you collected?
What kind of data have you collected?
0
reply
Report
#8
(Original post by mynameischloe)
Does anybody know how to calculate rate constant k using the arrhenius equation?
Does anybody know how to calculate rate constant k using the arrhenius equation?
(Original post by mynameischloe)
I worked out the initial rates of these reactions
I worked out the initial rates of these reactions
Or is it irrelevant now, as you got it after dragonkeeper999 hints?
0
reply
Report
#9
(Original post by mynameischloe)
I tested 5 different concentrations of hydrogen peroxide keeping catalyst concentration constant. I then tested 5 different amounts of manganese (IV) oxide keeping H2O2 constant. I worked out the initial rates of these reactions and the order is first in respect to both reactants.
I tested 5 different concentrations of hydrogen peroxide keeping catalyst concentration constant. I then tested 5 different amounts of manganese (IV) oxide keeping H2O2 constant. I worked out the initial rates of these reactions and the order is first in respect to both reactants.
0
reply
(Original post by itsije)
How did you vary the concentrations of Hydrogen Peroxide? I've looked almost everywhere for info and I'm still confused
How did you vary the concentrations of Hydrogen Peroxide? I've looked almost everywhere for info and I'm still confused
Posted from TSR Mobile
0
reply
Report
#11
(Original post by mynameischloe)
Hi, sorry for the very late reply! I just diluted down the standard 100vol hydrogen peroxide which they provided at school to get the concentrations I needed. I tested 0.2 0.4 0.6 0.8 and 1molar.
Posted from TSR Mobile
Hi, sorry for the very late reply! I just diluted down the standard 100vol hydrogen peroxide which they provided at school to get the concentrations I needed. I tested 0.2 0.4 0.6 0.8 and 1molar.
Posted from TSR Mobile
0
reply
Report
#14
I'm also doing this same experiment, I'm using manganese (IV) oxide as my catalyst. How did you work out the order of reaction?
Posted from TSR Mobile
Posted from TSR Mobile
0
reply
Report
#16
That's what I expect mine to be but how do I work out out from the data I have. I have done 5 experiments varying the concentration of h2o2. 5 experiments varying the amount of mno2. I'm currently doing experiments with varying temperature.
0
reply
X
Page 1 of 1
Go to first unread
Skip to page:
Quick Reply
