Chapter 1, Problem 1.127E

How many grams of Mn3O4 can be obtained from 1.00 g MnO2? how many ounces of Mn3O4 can be obtained from1.00 lb  MnO2?  Whatwt of Mn ore should  be taken so that the percentage of MnO2 in the ore can be found by multiplying by 5 to the number of centigrams og Mn3O4

Given the following data for Mass of test tube and stearic acid = 14.17 gMass of test tube = 11.40 gFreezing point of strearic acid = 69.59o CMass of weighing paper + naphthalene =1.230 gMass of weighing paper = 0.920 gFreezing point solution = 64.00o CKf = 4.5o C/m Determine the following1. mass of stearic acid in g (2 decimal places); 2.77g2. mass of naphthalene in g (2 decimal places); 0.31g3. freezing point depression (2 decimal places);  3.93oC4. molality of solution (3 significant figures);  _____5. moles of naphthalene (3 significant figures); _____6. molar mass of naphthalene, experimentally (3 significant figures);  _____7. % error if theoretical molar mass of naphthalene is 128.17 g/ mole, USE ABSOLUTE VALUE (3 significant figure);  _____

(a) A solution of 20.91 % by weight H2SO4 has a specific gravity of 1.150. What is the normality of this solution? (b) Water is added to dilute this solution to a solution of 3.03% by weight H2SO4 (SG= 1.020). What is the new normality of the resulting solution and how were they mixed? (Assume 100 mL of the original solution was used.)