Question

7. (1 mark) Complete the table below (where k is the true rate constant): Temperature 1/T In(k) (K) (K*') (units = ?) (unitless) 295.15 3.39x10 -3 .007914 M. - 4.839 303.15 3.30 x 10-3 -4860 mois -0.7215 ** 308.15 3.25 x 10-5 -4494 M's--0.7998 -|* | 313.15 3.19 x 10-3 1.2998 M's- 11-1.204 * Data from Part 2. **Data from Part 3. (2 marks) On graph paper (by hand, not using a computer), make a plot of In(k) vs. 1/temperature, and determine the value of E. (R = 8.31451 J mol" K'). Hand in your graph, and show your calculations in the space below. In(K) InCA)- Ea/(RT). 8. (1 mark) Using the values of E, and A from your graph, calculate the expected value of the rate constant for this reaction at 10°C below your value of room temperature (from Part 2). Does it seem that the 2-3x change in rate per 10°C change in temperature "rule of thumb" would apply to this reaction?

when i turn it in i can only do handwritten. but if you can explain your results from excel and how to calculate everything thats fine. its due tomorrow please help!!

Answer 1

One can use a trendline function available in excel considering 1/temperature as x axis and lnk as y axis .it will give you the equation of a line which have a slope equal to activation energy.thats it.

Value of K gets doubled if the temperature is 10degree celsius increased.it is calculated on the basis of temperature coefficient.

Using arhenius equation u can calculate the value of k..its very easy