the avg k is 0.016. How do I answer part 3?
the avg k is 0.016. How do I answer part 3? Question 5 Here are your...
Question #5 Here are the relevant data to determine the activation energy of the reaction. Rate constant (units not shown) Temperature (K) .13 293 0.11 308 Use the data above to determine the activation energy of the reaction? 83 kJ/mol Submit This value is not correct. Please check your calculations and try again. Question #6 Here are your data for trial of Lab 7 (the trial at room temperature without the catalyst): [103 initial (S203 initial Initial Rate .0023 M...
question 5,6 part 1 and 2 please
Question #5 Here are the relevant data to determine the activation energy of the reaction. Rate constant (units not shown) Temperature (K) .13 293 0.11 308 Use the data above to determine the activation energy of the reaction. -3628 kl/mol Submit Please enter your results to the correct precision. Question #6 Here are your data for trial of Lab 7 (the trial at room temperature without the catalyst): [103 initial (S2032 Jinitial Initial...
Table 3: Experimental Data for Part 2: Determination of Activation Energy k Time* T* [1] [S,0,?] Rate (M/s) (s) (C) (M) (M) Run 3 153 20.5 .0208 .0416 4.03*10^-6 4.65*10^-3 (Room T) Run 6 198 9 .0208 .0416 3.15*10^-6 3.64*10^-3 (Cool) Run 7 112 31 .0208 .0416 5.58*10^-6 6.45*10^-3 (Warm) Run 8 40 51 .0208 .0416 1.56*10^-5 1.80*10^-2 (Warmer) 1/T (1/K) In k Run 3 1/293.5 -5.37 Run 6 1/282 -5.62 Run 7 1/304 -5.044 Run 8 1/324 -4.02 20....
rates of chemical reactions
Plz help!! how do I find specific rate constant k, 1/T, In
K
thank you
Rates of Chemical Reactions: Report Form Rate Law Summary: (a) From your measurements, what are the reaction orders with respect to each of the three reactants H;O; HOO (b) What is the rate expression (rate law) for the uncatalyzed reaction? Rate = K LT-] [H202) (c) What is the total reaction order? 2 3. Effect of Temperature on the Reaction Rate...
Need help with the first picture. Data provided in pictures #2
& #3
Determining the Activation Energy and Collision Frequency Factor for Reaction 1 Part 1. Transfer the reaction rate for runs 9.12 from Data Sheet 3. Then calculate the rate constant (R) at each temperature based on the reaction orders determined in parts and Record the results in Tables * = 18,0 ->15.0416"5,0216" Equation 6 ->25 10 2. Calculate the natural logarithm of the rate constant. In ) and...
just one example/demonstration!
Data needed to be calculated is in highlighted in green boxes.
And I highlighted in red an equation (not sure if thats what you
use to calculate it) And ignore the lab instructions on completeing
a graph!! I already know how to do that in excel, just curious how
Ln (relative rate) and 1/T in K^-1 is calculated by hand*
here is the rest of that lab leading up to the question as I
know its typically...
Can you help me answer questions
3)a)i)ii)iii)iv).thank you so much for your help.These questions
are based on thermodynamics.I really appreciate your kindness and
help
Here are the updated questions.I provide you with bigger and
clearer pic for all the subparts.I hope you can help me.thanks a
lot.
CH (9) H20 (9) 186 1189 0,09 205 ThermodyWUM 301) Use the data in the foblo 600W- 1 0 Hon Compound AS CT mol KP write the b0/0 for the combustion of methane...
please correct me If I did anything wrong. im very confused on
this.
• Determining k in Beer's Law 2. Determining the equilibrium constant Test Tube No. Absorbance Test Tube No. Absorbance 0,060 이79 0.253 0319 0.400 0.120 0.268 0.361 0.461 0.695 Post Laboratory Questions 1. Complete the following table and calculate k-value for the Beer's Law. All concentrations should be in M. [Fe(SCN)2) Absorbance CA Test Tube No. Diluted Fe(NO3)2 (mL) 0 . 2 3 4 s Reference 1.0...