Given the percentage difference calculated in question 5, which of the following
ID: 540375 • Letter: G
Question
Given the percentage difference calculated in question 5, which of the following explanations would be the most logical reason for the error in the experiment?
21% difference
The student accidentally put to much methanol in the Erlenmeyer flask when heating the iodine. Causing the mass of product to be less than what was expected.
The student accidentally weighed out more iodine than what was recorded. Causing the mass of product to be more than what was expected.
The student accidentally forgot to place the zinc iodide product in a desiccator which allowed for the product to absorb water. Causing the mass of product to be more than what was expected.
No error, the reaction was successfully completed.
The student accidentally forgot to cover the top of the Erlenmeyer flask when heating the iodine solution causing some of the iodine to be removed from the solution. Causing the mass of product to be less than what was expected
1.
Given the following experimental data:
How much of the zinc reacted? 0.34
2.
Given the following experimental data and referring back to question 1( for mass of reacted Zn):
Calculate the following:
(a). moles of Zn -
(b). moles of I -
3. Using your answers in , in question 2, what is the empirical formula fo zinc iodide from this experimental data?
Zn4I5
4.
Using the empirical formula, in question 3, balance the following equation:
____ Zn(s) + ____ I2(s) ----> ___ ZnxIy(s)
What is the sum of the coefficents in the balance chemical equation?
20
5.
Given the following experimental data and data from question 1:
Calculate the percentage difference between mass of the product and mass of the reactant.
( Note: If percentage is negative, take the absolute value of it when answering the question)
21%
a.The student accidentally put to much methanol in the Erlenmeyer flask when heating the iodine. Causing the mass of product to be less than what was expected.
b.The student accidentally weighed out more iodine than what was recorded. Causing the mass of product to be more than what was expected.
c.The student accidentally forgot to place the zinc iodide product in a desiccator which allowed for the product to absorb water. Causing the mass of product to be more than what was expected.
d.No error, the reaction was successfully completed.
e.The student accidentally forgot to cover the top of the Erlenmeyer flask when heating the iodine solution causing some of the iodine to be removed from the solution. Causing the mass of product to be less than what was expected
1.
Given the following experimental data:
Before Reaction Massof empty Erlenmeyer flask 85.35g Mass of Zn and Erlenmeyer flask 86.90g Mass of iodine 1.65g After Reaction Mass of Erlenmeyer flask and unreacted zinc 86.56gHow much of the zinc reacted? 0.34
2.
Given the following experimental data and referring back to question 1( for mass of reacted Zn):
Before Reaction Massof empty Erlenmeyer flask 85.35g Mass of Zn and Erlenmeyer flask 86.90g Mass of iodine 1.65g After Reaction Mass of Erlenmeyer flask and unreacted zinc 86.56gCalculate the following:
(a). moles of Zn -
(b). moles of I -
3. Using your answers in , in question 2, what is the empirical formula fo zinc iodide from this experimental data?
Zn4I5
4.
Using the empirical formula, in question 3, balance the following equation:
____ Zn(s) + ____ I2(s) ----> ___ ZnxIy(s)
What is the sum of the coefficents in the balance chemical equation?
20
5.
Given the following experimental data and data from question 1:
Mass of zinc iodine reaction product 1.75gCalculate the percentage difference between mass of the product and mass of the reactant.
( Note: If percentage is negative, take the absolute value of it when answering the question)
21%
Explanation / Answer
The student accidentally forgot to cover the top of the Erlenmeyer flask when heating the iodine solution causing some of the iodine to be removed from the solution. Causing the mass of product to be less than what was expected. This isthe most logical reason for 21 % difference .
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