A calorimety lab can be summarized as follows: 2HCl(aq) + K2CO3(s) --> 2KCl(s) +
ID: 823567 • Letter: A
Question
A calorimety lab can be summarized as follows:
2HCl(aq) + K2CO3(s) --> 2KCl(s) + H2O(l) + CO2(g)
In trial 1 we combine 30ml/30g of the HCL with roughly 2.60g of K2CO3 (the experiment told us to use between 2.50 and 3.00g). The temperature went from 21 degrees celcius (starting temperature) to 24 degrees Celsius (after the roughly 2.60g of K2CO3 was added). Obviously, with this information we can calculate our q value, and also our delta H for the reaction. However, what If we were asked to calculate the heat change if 1mol of potassium carbonate (K2CO3) was used? Could we simply substitute our delta H for the reaction into our formula for q since we are dealing with constant pressure? If not, how would we calculate heat change if 1 mole (instead of only 2.60g) of potassium carbonate were used?
P.s. This isn't something out of a Chem110 course - it is Gr. 12 University Chemistry - still high school. Thanks.
Explanation / Answer
yes you can use delta h as q value by hess law and here u are dealing with moles instead of weight in grams as in previous case;so use standard molar enthalphy of formation values and apply hess law to obtain delta h of reaction
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