B. Formula of a Hydrate1. Mass of crucible32.162. Mass of crucible and hydrate40.943. Mass of crucible and anhydrateg36,483a Mass of crucible and anhydrate (second heating)Calculations4. Mass of hydratet76 g5. Mass of anhydrate4ろと86. Mass of water lost4.4687. Percent water (Show calculations.)%8. Moles of water (Show calculations.)moles9. Moles of salt (anhydrate) (Show calculations.)moles10Ratio of moles of water to moles of hydrate11Formula of hydrateMgSO, •H2OQuestions and ProblemsQ5 Using the formula you obtained in B11, write a balanced equation for thedehydration of the MgSO, hydrate used in the experiment.

Since you have posted multiple sub-parts, we will solve first three sub-parts for you. To get…

B. Formula of a Hydrate 1. Mass of crucible 32.16 2. Mass of crucible and hydrate 40.94 3. Mass of crucible and anhydrate 36.48 3a Mass of crucible and anhydrate (second heating) Calculations 4. Mass of hydrate 5. Mass of anhydrate 4ると8 6. Mass ofwater lost ササー 7. Percent water (Show calculations.) moles 8. Moles of water (Show calculations.) moles 9. Moles of salt (anhydrate) (Show calculations.) mle

B. Formula of a Hydrate 1. Mass of crucible 32.16 2. Mass of crucible and hydrate 40.94 3. Mass of crucible and anhydrate 36.48 3a Mass of crucible and anhydrate (second heating) Calculations 4. Mass of hydrate 5. Mass of anhydrate 4ると8 6. Mass ofwater lost ササー 7. Percent water (Show calculations.) moles 8. Moles of water (Show calculations.) moles 9. Moles of salt (anhydrate) (Show calculations.) mle

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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SOLVE THE FOLLOWING: I. Find the molar mass of the given elements or compounds. Express your answers in g/mol. Show your solution. 1. Al tesnetoW otod 2. C12H22011 Insmel3 edf io 22om oimotA Inem 3. MgCl2 loM 220M oimotA Insr umo 10.01 umb 0.C lomp fo.cr 4. C2H4 OM YoloM
One mole of 0, has a mass of 16.0 g. Select one: O True O False
Quantity 1. Mass of crucible + cover 2. Mass of crucible + cover + Magnesium 3. Mass of Magnesium 4. Mass of crucible + cover + magnesium oxide 5. Mass of magnesium oxide 6. Mass of oxygen that combined with the magnesium 7. Atomic mass of magnesium 8. Atomic mass of oxygen 9. Moles of magnesium 10. Moles of oxygen Subtract # 2 - #1 Subtract #4 - #1 Subtract #4 - #2 From the periodic table From the periodic table Divide #3/#7 (In other words, divide the grams of magnesium by 24.3 to get the moles of magnesium) Your value Find the simplest whole number ratio 11. Empirical formula of magnesium between #9 and # 10. Those whole oxide based on this data numbers become of the subscripts of the formula* 20.00 g 24.86 g 28.06 g 24.3 16.0 moles of Mg Divide #6/#8 (In other words, divide the moles of moles of O oxygen by 16.0 to get the moles of oxygen *For example, if the moles of Mg were found to be 2.0 moles, and the moles of O were found to be 6.0 moles, then you would write the following:…
Determine the empirical formula of a compound that has the following mass % composition: 47.31% C, 10.59% H and 42.10% S. Empirical formula: Edit View Insert Format Tools Table 12pt Paragraph v BIU AT²V 30. 聞く

a.) The percent composition of an unknown compound is 48.71% C, 30.73% O, 11.96% N, and 8.60% H. What is its empirical formula? Show your work. b.) We have an oxide of cobalt (the substance contains only Co and O) that is, by mass, 58.93% Co. What is its empirical formula?
Mass of crucible, lid, and magnesium oxide ____19.41 g____ Mass of empty crucible and lid after heating _____15.05 g___ Mass of magnesium oxide ______________g_ Determine the mass of magnesium oxide
A mixture of 197.1 g of P and 203.6 g of O, reacts completely to form P0, and P010: Find the masses of P,0, and PO10 that are formed by the reaction. mass of P,06: 174.7 112.8 mass of PO10: 4 Incorrect
4. Calculate grams P in 97.6grams barium phosphate.
A sample of bromine has a mass of 40.8 grams. a. How many Br atoms are there in the sample? atoms b. How many Br2 molecules are there in the sample? molecules Submit Answer Retry Entire Group 9 more group attempts remaining a. What is the mass of 1.74 x 1024 atoms of oxygen? grams b. What is the mass of 3.02 x 1023 molecules of oxygen? grams grams values if needed for this question. a. What is the mass of 1.46 x 1024 atoms of iodine? grams b. What is the mass of 1.88 x 1024 molecules of iodine? vay Me Reierences to access important values if needed for this question. a. What is the mass in grams of 1 zinc atom? grams b. The number of atoms in 60.9 grams of zinc would be Avogadro's number.
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Please
Given 9.4 moles of Ca, the mass can be calculated as: (Hint: Molar mass of Ca is 40 g/mol). O a. 9.4/40 O b. 9.4*40 c. 9.4-40 O d. 9.4+40