9.) As mentioned below, you are required to design your ownprocedure for determining the heat of dissolution of your chosensalt with a coffee cup calorimeter. Answer the following questionsand consider them in designing this procedure:

     a.) When you find your initialtemperature T_i, should you take one measurement from thethermometer as soon as you place it in the water in thecalorimeter? Why or why not? If not, what should you doinstead?

     b.) Do you expect the temperature ofthe water in the calorimeter to rise, fall, or stay the same afteryou add your salt? If the temperature will change, will it continueto change indefinitely or not?

     c.) How will you know your dissolvedsalt solution has reached it's maximum or minimum temperature, i.e.what will you observe in your data to indicate this hashappened?

     d.) Should you repeat your experiment?Why or why not? If so, what could you change from trial to trial?Give two possible suggestions, and determine which one you shouldchange (as well as which one you should not!) in any subsequenttrials you decide to perform.

*Information previously calculated is below*

1. Calculate the amount of heat (q) produced by the combustionof 4.05 g CH₄ (ΔH_comb =-890.4 kJ).

225.38 kj

2. Consider that the 4.05 g methane is burned and all of theheat from this combustion is absorbed by 1.0 kg of 20°C water (use 4.18 g^-1 ºC^-1for the specific heat of the water). What would be the finaltemperature of the water?

73.8°C