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Lecture

tutorial jun 13.docx

2 Pages
108 Views

Department
Chemistry
Course Code
CHEM 1000
Professor
Hameed A.Mirza

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Description
1. Aqueous silver ion reacts with aqueous chloride ion to yield a white precipitate of silver chloride. Ag + cl agcl When 10.0 ml of 1.00 M AgNo is adde3 to 10.0 ml of 1.00 M Nacl solution at 25C in a calorimeter a white precipitate of Agcl forms and the temperature of the aqueous mixture increases to 32.6C Assuming the specific heat of the aqueous mixture is 4.18 J/gC the density of the mixture is 1.00 g/ml, calorimeter absorbs negligible heat. Calculate ∆H in kJ in the reaction. Ans. * Balance the equation first! In such cases m = 20.0 ml x 1 g/ml = 20 g ∆T = 32.6C – 25.0C = 7.6C 2 q = 4.18 J/gC x 20.0 g x 7.6C = 6.4 x 10 J moles of Ag = 10.0 ml X (1.00 mol Ag / 1000 ml ) = 1.00 X 10 mol Ag 2 + Therefore, moles of AgCl Heat evolved / mole AgCl = 6.4 X10 J / (1.00 X 10 mol AgCl) = -64 KJ/ mol Agcl *Either mention heat is evolved or put the negative sign 2. Oxyac welding torches burn acetylen
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