mass of empty cruciole = 31.06ua. mass of Crucible+ Mg= 31.034 t0.001 1) Determine the empirical formula of Mgo based on your data. Follow the steps used in the introduction for finding the empirical formula of NO, (mg) Csl ribbion 6.5o mass of crucible + MqO= 31.970 q t0.0 STEP 1: Find ghåons many grams of Mg were in your MgO sample? (see final results); 31.434-31.644= 0.579 0.002 How many grams dt O in your Mgo sample? This will be a subtraction since you know mass of Mg and mass of Mgo. .57 =0.023 mol (mg) 13369 24.31 STEP 2: Find Motrvert grams of Mg to moles: 6.906 - 0.570.336 31.970 - 31.do4 =6.906 Convert grams of O to moles: 334 Onygen = 0.021 mol 16.60 STEP 3: Find FBivideeach by the smallest number to get a whole number ratio for the formula:
mass of empty cruciole = 31.06ua. mass of Crucible+ Mg= 31.034 t0.001 1) Determine the empirical formula of Mgo based on your data. Follow the steps used in the introduction for finding the empirical formula of NO, (mg) Csl ribbion 6.5o mass of crucible + MqO= 31.970 q t0.0 STEP 1: Find ghåons many grams of Mg were in your MgO sample? (see final results); 31.434-31.644= 0.579 0.002 How many grams dt O in your Mgo sample? This will be a subtraction since you know mass of Mg and mass of Mgo. .57 =0.023 mol (mg) 13369 24.31 STEP 2: Find Motrvert grams of Mg to moles: 6.906 - 0.570.336 31.970 - 31.do4 =6.906 Convert grams of O to moles: 334 Onygen = 0.021 mol 16.60 STEP 3: Find FBivideeach by the smallest number to get a whole number ratio for the formula:
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I'm stuck on step 3. find the formula - Divide each by the smallest number to get while number ratio for the formula
With the information I've provided under attachments can you help?
I don't know how to calculate the smallest number to get the ratio for the formula.
Transcribed Image Text:10:26 PM Thu Apr 8
30% O
Module 6; Empirical Formula of Magnesium Oxide
0O
X Module 1; Measurement (and CHEM...
X Module 2; Classifying Matter and Ch...
fallacy quiz
Module 6; Empirical Formula of...
31.06U g to.001
mass of Cvuciblet Mg=
31.034
mass of empty Crucible =
1) Determine the empirical formula of MgO based on your data. Follow the steps used in the introduction for
finding the empirical formula of NO,.
mg)
Csrl ribbion O.50
mass of crucible t MqO= 31.970 9 t0.001
STEP 1: Find graows many grams of Mg were in ybur MgO sample?
(see final results);
6.759
31.434-31.644= 0.579,
t 0.002
How many grams of O in your MgO sample?
This will be a subtraction since you know mass
of Mg and mass of MgO.
.57
=0.023 mol (mg)
13369
24.31
STEP 2: Find Mobeevert grams of Mg to moles:
6. 906 - 0.Š770.336
31.970 - 31.dol = 6.906
Convert grams of O to moles:
334
0.021 mol Okygen
16.00
STEP 3: Find FDiwidtaeach by the smallest number
to get a whole number ratio for the formula:
2) Determine the theoretical formula of MgO using the periodic table. To do this: find the most stable ion of
magnesium and the most stable ion of oxygen. Use that to predict the formula for magnesium oxide:
• Mg ion ®
• O ion R
• Formula for magnesium oxide
3) Compare what you got in #1 to what you should have got in #2. How close were you? How might you
explain the difference?
Post-Lab Question
1) Hypothetical Data for Analysis
An oxide of iron is 69.94% iron by mass. Calculate its empirical formula and determine the name of the ionic
compound. (Hint: assume you have a 100 g sample of the oxide of iron. How many grams would be iron?
Then how many grams would be oxygen? Convert those to moles. Find the ratio. Find the nearest whole
number ratio). Then determine its name.
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