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4.4LAB #10Behavior of Copper in a Solution of Silver NitrateJennie Chang (even)Allison Yee (odd-Partner)Mackenzy Doniak (even-Partner)January 14, 2011CALCULATIONS
1. Calculate the number of moles of Cu that reacted and entered the solution.(1.48 g of Cu) /1 x (1 mol / 63.5 g of Cu) = .023 moles of Cu that reacted andentered the solution2. Calculate the number of moles of Ag formed.(.64 g Ag/1) x (1 mol/ 108 g Ag) = .01 moles of Ag formed3. Determine the ratio, mole Ag/ mole Cu.4. Determine and write a balanced equation for this reaction. (Singledisplacement, Copper(II) )Cu+ AgNO3Ag + Cu(NO3)2Cu + 2gNO32Ag + Cu(NO3)25. What is the ratio, moles Ag/moles Cu according to the balanced equation.(2 g Ag/1) x (1 mol/ 214Ag) = .01 moles of Ag(1 g Cu/1) x (1 mol/63.5 g Cu) = .023 moles of Cu6. Calculate the % error.Equation:True Value – Experimental Value / True Value × 100 = Percent Error[(.01/.023)-(.01/.023)]/ (-.013) x 100 = 0%DISCUSSION