PLEASE ANSWER ALL 4 OF THE CONCLUSION QUESTIONS Conclusion Explain how the obser
ID: 535869 • Letter: P
Question
PLEASE ANSWER ALL 4 OF THE CONCLUSION QUESTIONS
Conclusion Explain how the observations that were made were indicative of a chemical reaction. Also, explain which of the two reactants the limiting reactant Use the number of moles of zinc atoms and iodine atoms to calculate the empirical formula of the product. Base your answer on the mass of zinc consumed and the mass of iodine consumed. Is this what you expected? Discuss the Law of Conservation of Mass. Is it always obeyed? If not, when? If the mass of product is too high, what caused this? If the mass of product is too low, what caused this? What errors were made during this experiment? As an example, comment on: if some unreacted zinc was spilled, how would this affect the ratio of moles (think carefully about this)? List at least two other errors. How did each error affect the ratio of moles of zinc to moles of iodine used? Reference: Wells N. Bochmann, E. J Chem. Educ 1977, 54, 386
Explanation / Answer
1. The chemical reaction occured, because the color of iodine disappeared from the solution when ZnI2 is formed. Limiting reactant is iodine.
2. moles Zn = 1.50/65.38 = 0.023 mol
moles I2 = 2.60/253.81 = 0.01 mol
So,
Zn = 0.023/0.01 = 2
I2 = 0.01/0.01 = 1
empirical formula = ZnI
No we expected a ZnI2 formula.
3. Law of conservation of mass suggest mass is never created or destroyed but remains the same overall. The law is obeyed. If the mass of product is too high, more I2 was added then needed. If mass is too low, less amount of limiting reactant I2 was added.
4. Errors, like spilled zinc would lower the yield of the reaction as lesser Zinc was left to react and form product. Excess I2 added would give higher product weight. Moles of Zn would be lower than moles of I2. If not all the solution after reaction is transferred, the product yield would be lower, Zn moles would be higher, I2 moles would be lower.
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