## Question

###### When i turn it in i can only do handwritten. but if you can explain your...

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!!

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?

## Answers

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

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