Overview
1. Open a new tab/excel file and copy and paste your molecule's temperature dependent heat capacity data over. Be sure to also copy and paste Cp(T) equation and coefficients for high and low T ranges, if applicable.
2. Dividing each term in the Cp(T) equation by T, write the new Cp(T)/T equation.
3. Using the lecture notes for solved intregral terms, write the integrated equation of your Cp(T)/T equation (this should have as many terms as your original Cp(T) equation).
4. Create a column labeled DS with proper units and another column labeled S(T2) with proper units.
5. Format the integrated equation from step 3 into the DS column, setting T1 always equal to 298 K. Remember to lock the T1 value and the coefficients, allow T2 to change.
Hint: the value for this column at 298 K should be 0.00!
Hint 2: remember to change the coefficients when your temperature range changes, if applicable.
6. Find, record, and cite the source for the standard entropy of your molecule. Unlike standard enthalpy of formation, no molecule has a standard entropy value of zero. Copy and paste the value into a cell on your excel page and remember to include proper units.
7. Set the S(T2) column to equal the sum of the DS column at each temperature plus the constant standard entropy value from step 6. Remember to lock the value from step 6.
You should now have change in entropy and absolute entropy values for each of your temperatures above 298 K.
8. Graph the change in entropy vs T and the absolute entropy vs T (two separate graphs or one overlayed graph ok; x axis is temperature).
9. Find the best fit trendline for each of these and remember to use proper labels for the trendline (scientific, four decimal places).
Repeat for each molecule in your equation. See video for help but I strongly recommend trying to complete first on your own so you're building your own understanding.