Lab 10 Behavior of Copper in a Solution of Silver Nitrate - 4.4 LAB#10 Behavior of Copper in a Solution of Silver Nitrate Jennie Chang(even Allison

Lab 10 Behavior of Copper in a Solution of Silver Nitrate -...

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4.4 LAB #10 Behavior of Copper in a Solution of Silver Nitrate Jennie Chang (even) Allison Yee (odd-Partner) Mackenzy Doniak (even-Partner) January 14, 2011 CALCULATIONS
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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 and entered the solution 2. Calculate the number of moles of Ag formed. (.64 g Ag/1) x (1 mol/ 108 g Ag) = .01 moles of Ag formed 3. Determine the ratio, mole Ag/ mole Cu. 4. Determine and write a balanced equation for this reaction. (Single displacement, Copper(II) ) Cu+ AgNO3 Ag + Cu(NO3)2 Cu + 2gNO3 2Ag + Cu(NO3)2 5. 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 Cu 6. Calculate the % error. Equation: True Value – Experimental Value / True Value × 100 = Percent Error [(.01/.023)-(.01/.023)]/ (-.013) x 100 = 0% DISCUSSION
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  • Spring '10
  • Stevens
  • Chemistry, Mole, 0%, electronic device, Jennie Chang, Allison Yee

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