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Empirical formula 12456ref, Summaries of Chemistry

American University of BeirutChemistry

Empirical formula 123456vussg qcu

Typology: Summaries

2022/2023

Uploaded on 02/23/2024

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Chemistry 101L
Experiment 2: Empirical Formula and Avogadro’s Number Pre-
lab Assignment
Name:_________________ Date:___________________
ID #:__________________ Section:_________________
1. An analysis shows that 5.85 g of a chromium metal combines with oxygen to form
8.62 g of chromium oxide. What is the empirical formula of the compound?
2. The formula for rust can be represented by Fe2O3.
a) How many moles of Fe2O3 are present in 24.6 g of the compound?
b) How many moles of Fe are present in 24.6 g of the compound?
c) How many atoms of oxygen are present in 24.6 g of the compound?
3. Zinc metal has a hexagonal close packed structure. Calculate the volume of a unit cell of Zn in cm3.
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Chemistry 101L Experiment 2: Empirical Formula and Avogadro’s Number Pre- lab Assignment Name:_________________ Date:___________________ ID #:__________________ Section:_________________

1. An analysis shows that 5.85 g of a chromium metal combines with oxygen to form 8.62 g of chromium oxide. What is the empirical formula of the compound? 2. The formula for rust can be represented by Fe 2 O 3. a) How many moles of Fe 2 O 3 are present in 24.6 g of the compound? b) How many moles of Fe are present in 24.6 g of the compound? c) How many atoms of oxygen are present in 24.6 g of the compound? 3. Zinc metal has a hexagonal close packed structure. Calculate the volume of a unit cell of Zn in cm^3.

Chemistry 101L Experiment 2: Empirical Formula and Avogadro’s Number Lab Report Name: _____________________ Date: _________________ Purpose of the experiment: Part 1 Data : Mass of 125 mL Erlenmeyer flask = Mass of 125 mL Erlenmeyer flask + zinc granules = Mass of 125 mL Erlenmeyer flask + zinc granules + iodine= Mass of 150 mL beaker = Mass of Erlenmeyer flask + unreacted zinc = Mass of beaker + zinc iodide = Calculations : Mass of zinc granules = Mass of iodine = Mass of iodine + zinc (before reaction) = Mass of unreacted zinc = Mass of zinc iodide = Mass of reacted zinc = Mass of reacted iodine + reacted zinc = Mass of unreacted zinc + product = Moles of reacted zinc = Moles of reacted iodine = Ratio of moles of one element to the other = Empirical formula of zinc iodide = Questions

1. Write a balanced chemical equation for the reaction of zinc with iodine. 2. Show by referring to calculations whether mass is conserved in a chemical reaction.

Questions

1. How many moles are in 1.5 g of zinc? How many atoms? 2. If the displaced water in the volumetric flask is not removed completely to the mark, what effect will that have on the calculated density of zinc? Explain