n this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the heat of reaction for this reaction, in sig figs?
n this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the heat of reaction for this reaction, in sig figs?
q (reaction) = – q (solution) + – q (calorimeter)
q (reaction) = – (4.368 g + 35.5 g) x (4.184 J/g℃) x (27.086365℃ – 20.00℃)
+ – (29.4 J/℃) x (27.086365℃ – 20.00℃)
q (reaction) = – 1182.060326 J + – 208.339131 J
q (reaction) = – 1390.399457 J
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