7. An organic chemist needs to quantitatively oxidize an unsaturated compound into a diol. The reaction uses potassium permanganate , the formula for the unsaturatec compound is C17H2604, the solution is acidic and the formula for the product is C17H24O6. If his/her sample weighed 1.506 grams and required 39.75 ml of a standardized KMNO4 solution, what was the molarity of the KMNO4 solution?

7. An organic chemist needs to quantitatively oxidize an unsaturated compound into a diol. The reaction uses potassium permanganate , the formula for the unsaturatec compound is C17H2604, the solution is acidic and the formula for the product is C17H24O6. If his/her sample weighed 1.506 grams and required 39.75 ml of a standardized KMNO4 solution, what was the molarity of the KMNO4 solution?

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...

See similar textbooks

Similar questions

If exactly 4.089 moles of propanol (C3H8O) is combusted in the presence of excess oxygen what is the mass of O2 used in the reaction? The molecular weights of all reactants and products are: C3H8O: 60.09 g/mol O2: 31.998 g/mol H2O: 18.016 g/mol; CO2 : 44.01 g/mol. Enter your answer in the units of g, do not enter the unit itself.
This is part of a continuing problem with the previous carbohydrate sample. Use the previous data in this part. 1) A 12.915 g carbohydrate sample composed of CHO was analyzed by combustion analysis from which was obtained 18.942 g CO2 and 7,74 g H2O. The molar mass of the sample was found to be 455.32 g/mole by independent analysis. How many repeat units are in this molecule? Input the numeric value here. Hint: This is a whole number value. Hint: The repeat units are determined by the ratio of the empirical formula molar mass to the molar mass of the sample; the empirical formula is determined by the ratio of moles of the compound's elements. 2) What is the molecular formula? Include this for your notes for personal practice. Table molar mass (g/mol): C 12.00, O 16.00, H 1.008.
Help needed with question 1 of the image attached
Please help with this question: Thanks!!! C15H24 (39.288g) was oxidized to C9H6O6, using an excess of oxidizing agent. Calculate the theoretical yield of the organic product a) in moles, and b) in grams.
a) NH4OH + HCI HCI → Type of reaction b) Na2S + CUSO4 → Type of reaction Туре с) ZnCl2 + N2OH → Type of reaction
In synthesizing aspirin, a student used 5.324 g of salicylic acid and excess acetic anhydride. After recrystallization, the product weighed 6.362 g. Calculate the percent yield of aspirin.
Nicotine is a naturally produced alkaloid and is widely used recreationally as a stimulant that produces pleasing effects in brain making it addictive. It is composed 74.017% C, 8.714% H and 17.269% N. In 1.00-g sample of nicotine contains 6.163X10^-3 moles. Determine its molecular formula? Please show the complete solution and write clearly. Thank you.
Organic Chemistry II: When nitrating Methyl benzoate, which compound is the limiting reactant?