Rates+of+Reactions

__Introductory Activity:__
Monitoring the mass of the coca-cola over time:


 * Time (s) || Mass (g) ||
 * 0 || 86.730 ||
 * 10 || 86.718 ||
 * 20 || 86.710 ||
 * 30 || 86.702 ||
 * 40 || 86.697 ||
 * 50 || 86.692 ||
 * 60 || 86.686 ||
 * 70 || 86.685 ||
 * 80 || 86.680 ||
 * 90 || 86.679 ||
 * 100 || 86.676 ||
 * 110 || 86.673 ||
 * 120 || 86.671 ||
 * 130 || 86.667 ||
 * 140 || 86.664 ||
 * 150 || 86.661 ||
 * 160 || 86.660 ||
 * 170 || 86.658 ||
 * 180 || 86.656 ||
 * 190 || 86.651 ||
 * 200 || 86.650 ||
 * 210 || 86.648 ||

Put all of this data into excel. Create a new column and determine the total mass of CO2 formed for each time value. Convert mass of CO2 into moles of CO2. Put the number of moles of CO2 into the new column.

a) Plot Moles of CO2 produced against time. b) Create another column next to the moles of CO2 produced for moles of H2CO3 decomposed. c) Plot Moles of H2CO3 decomposed against tme. b) Calculate the average rate of CO2 production between t= and t= c) Calculate the instantaneous rate of CO2 production at t=0 d) Calculate the instantaneous rate of CO2 production at t= d) Write out the balanced chemical reaction that is occuring e) For the same times as selected for questions b), c), and d), determine the instantaneous rate of decomposition of H2CO3.

Graphs: