Part 2 post lab 4 - =absolute value of...

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Part 2 This method in determining the heat of formation of solid NH 4 NO 3 is very reliable. After calculating the heat lost by the calorimeter, that is used for the entire experiment, when calculating the q (rxn) and the change in heat of both reactions, that value can be used to counter the heat lost. Therefore in calculating my heat of formation of solid NH 4 NO 3, the actual value was very close to that of the theoretical value. In fact my % error was: %error=absolute value of ((experimental value – accepted value)/accepted value)x100
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Unformatted text preview: =absolute value of ((-366.8-(-365.6))/-365.6)x100 =.01% error Since experimental errors were minimized using the heat lost by the calorimeter, my percent error was minimized. Other contributors to this value were the repeated trials and related reactions. By doing multiple trials and taking the average of the two, better observations and data can be taken. Ultimately minimizing error and the value calculated above....
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