CHM 103 Lecture Notes - Lecture 14: Calorimetry, Sodium Hydroxide, Joule

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Measurement of heat transfer and reaction enthalpies q = n * cp * t n = moles (cid:3040)(cid:3039) (cid:4667) Cp = molar heat capacity ( q = m * cs * t m = mass. Isolating the system you are studying from the surroundings. Depending on how food the insulator is, the calorimeter will probably absorb some of the heat. Q h (when running in constant temperature) 100 ml of water at 50 oc is mixed with 100 ml of water 20 oc. The final temperature of water is 33 oc. Ideally, the final temperature would be 35 c (the number exactly between 20 c and 50 c). Heat lost (50 c): (100g) (4. 184 ) (50 c-33 c) = 7113 j. Heat gained (20 c): (100g) (4. 184 (cid:4667) (20 c - 33 c) = 5439 j. Heat gained by calorimeter: 7113 j 5439 j = 1674 j (where ccal = calorimeter heat capacity) qcal = ccal t.

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