S2O82-(aq) + 2I-(aq) ----------> 2SO42-(aq) + I2(aq) (I)
Rate = k [S2O82-]x [I-]y
Rate1 = k [S2O82-]x [I-]y
ƒ´ [S2O82ƒ{]
Rate = ƒ{ƒn -------------
ƒ´ƒnt
Experiment data
Experiment: 0.20M NaI,0.20M NaCl, 0.010M Na2S2O3,2% Starch,0.20M K2SO4, 0.20 M K2S2O8
Used 2ml of each solution for the experiment. Need help calculating these:
Calculated concentration of S2O82ƒ{ _______________ mol/L
Calculated concentration of Iƒ{ _______________ mol/L
Total elapsed time (ƒ´t) _______153sec
Rate of reaction _______________ M/sec
(from mathematical rate expression)
Rate constant, k _______________ sec-1
I can't read your post. the script f, script f' and brackets ({ and }) don't make sense.
To calculate the concentration of S2O82- and I- and the rate of reaction, you need to use the given experimental data and the rate expression.
From the balanced chemical equation (I), we can see that the stoichiometric coefficient ratio between S2O82- and I- is 1:2. Therefore, the rate expression can be simplified to:
Rate = k [S2O82-] [I-]^2
Now let's plug in the values from the experiment:
- Concentration of S2O82-: 0.010 M (Given)
- Concentration of I-: 0.20 M (Given)
To find the total elapsed time (Δt), you should consider the time it took for the reaction to occur, which is given as 153 seconds.
To calculate the rate of reaction, divide the change in concentration of the reactant (S2O82-) by the total elapsed time:
Rate = [S2O82-]t / Δt
However, we need to note that the given experiment does not provide the initial and final concentrations of S2O82-. So without that information, we cannot calculate the exact rate of reaction or the rate constant (k).