Data Table 1. Mass of flask +iodine - Mass of empty flask Mass of iodine used 83
ID: 538222 • Letter: D
Question
Data Table 1. Mass of flask +iodine - Mass of empty flask Mass of iodine used 83.310 3.388g 2. 002 2.00c Mass of zinc used Observations after addition of methanol: The cotor immadia ations after addition of methanol: d e Zinc iodide is produced in the reaction. Where is it? At the bothom of lask Data Table 2. //0.75 8 109 (o45 1.11302 Mass of beaker+crystals - Mass of beaker Mass of crystals formed Data Table 3 Mass of flask + solid; 1t weighing Mass of flask +solid; 2hd weighing Mas of fask + solid, 5" weighing GF 72641 82,0410 necessary) unnucos Mass of excess reactant recovered -1.253 a What color are the crystals that formed in the beaker? uhiteExplanation / Answer
Step I
Mass of Iodine Used = 83.39 - 81.388 = 2.002 g
Moles of Iodine used or reacted = 2.002 / 253.809 = 0.007888
Step II
Moles of Zinc reacted = Moles of ZnI2 formed = 1.113 / 319.22 = 0.003487
Check your molar mass of ZnI2 again!
Mass of Zn reacted = 0.003487 x 65.38 = 0.228 g
Step III
Moles of I- reacted = 2 x Moles of ZnI2 formed = 2 x 0.003487 = 0.006974
Step IV
Use the formula with the corrected values to get the emperical formula for Zinc Iodide.
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