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. 10:26 PM Thu Apr 830% OModule 6; Empirical Formula of Magnesium Oxide0OX Module 1; Measurement (and CHEM...X Module 2; Classifying Matter and Ch...fallacy quizModule 6; Empirical Formula of...31.06U g to.001mass of Cvuciblet Mg=31.034mass of empty Crucible =1) Determine the empirical formula of MgO based on your data. Follow the steps used in the introduction forfinding the empirical formula of NO,.mg)Csrl ribbion O.50mass of crucible t MqO= 31.970 9 t0.001STEP 1: Find graows many grams of Mg were in ybur MgO sample?(see final results);6.75931.434-31.644= 0.579,t 0.002How many grams of O in your MgO sample?This will be a subtraction since you know massof Mg and mass of MgO..57=0.023 mol (mg)1336924.31STEP 2: Find Mobeevert grams of Mg to moles:6. 906 - 0.Š770.33631.970 - 31.dol = 6.906Convert grams of O to moles:3340.021 mol Okygen16.00STEP 3: Find FDiwidtaeach by the smallest numberto 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 ofmagnesium and the most stable ion of oxygen. Use that to predict the formula for magnesium oxide:• Mg ion ®• O ion R• Formula for magnesium oxide3) Compare what you got in #1 to what you should have got in #2. How close were you? How might youexplain the difference?Post-Lab Question1) Hypothetical Data for AnalysisAn oxide of iron is 69.94% iron by mass. Calculate its empirical formula and determine the name of the ioniccompound. (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 wholenumber ratio). Then determine its name.

Answered: Image /qna-images/answer/3cfcbafd-0ffe-40dd-9a2f-1e643be31d24.jpg

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:

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 1P

See similar textbooks

Similar questions

a concentrated H2SO4 has the following composition specific gravity 1.84 and purity of H2SO4 is 97 percent by weight. express in mole/L
Q3 / The solubility of sodium chloride NaCl in water at 290 Kis 35.8 kg / 100 kg of water. Express the solubility as the following: 1. Mass fraction and the mass percent of Naci 2. Mole fraction and mole percent of NaCl 3. kmol of NaCl per 1000 kg of water Note: molecular weight of NaCl = 135.8, and water = 18.016
Prepare 1500mL of 0.5N H2SO4 solution with specific gravity of 1.84g/mL and assay of 97%
A 18 g of unknown organic sample was dissolve in 756 mL of benzene. The boiling point of benzene was increased by 3.36oC. As the first step of analysis, determine the moecular weight of the unknow sample? Kb of benzene= 2.64oC/m Bb of benzene = 80.09 oC density of benzene = 0.874 g/mL at 25 °C Answer in whole number, no units required.
A 100 g soil containing 20% smectitie mineral matter was mixed with 150 mL solution containing 0.10 M Pb. CEC of pure smectitie is 110 emol(+)/kg. CEC of the soil (cmol(+)/kg) is:
Calculate the values of vrms, vmp, and vmean for Cl2 (70.90 g mol-1) at 25 °C
The following molarities were calculated from replicate standardization of a solution: 0.5022, 0.5022, 0.5021, 0.5008, upper limit of the 95% confidence interval?
The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole number
The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What CASE does this experiment satisfy?
A spent 1.0 percent caustic soda solution (ρNaOH = 8.42 lb/gal) with a volumetric flow rate of 3.0gpm is to be neutralized using either sulfuric acid or hydrochloric acid. First, determine the massflow rate (lb/day) of NaOH in the spent caustic soda solution, and then use that value todetermine the stoichiometric amounts (lb/day) of:1. H2SO4 required for neutralizing the OH− ions contributed by the spent caustic soda.[Hints: (1) write the balanced chemical equation for the acid-base reaction betweenNaOH and H2SO4, and use it to establish the stoichiometric weight ratio H2SO4 : NaOH.]2. HCl required for neutralizing the OH− ions contributed by the spent caustic soda. [Hints:(1) write the balanced chemical equation for the acid-base reaction between NaOH andHCl and use it to establish the stoichiometric weight ratio HCl : NaOH.]
Determine the percentage Fe in a sample of limonite from the following data:Sample : 0.5000g ; KMnO4 used = 50.00 ml ; 1.000ml of KMnO4 is equivalent 0.005317 g Fe,FeSO4 used = 6.00 ml; 1.000ml FeSO4 is equivalent 0.009200 g FeO ( ans 44.59 %)
A salt solution (30% Na2CO3) weighing 1ton iscooled to 20C where the salt crystallizes asdecahydrate. What will be the crystal yield ifthe solubility is 21.5 kg anhydrous Na2CO3/100kg water? (assume that 3% of the totalsolution is lost by evaporation)