An organic compound (with an index of hydrogen deficiency of 1), containing only carbon, hydrogen, and oxygen was burned in excess oxygen. When 12.915 g of the organic compound is burned, this produced 18.942 g carbon dioxide and 7.749 g of water. The organic compound was reacted with 3 moles of trimethylsilyl chloride (TMSCI) as protecting agent (used to protect alcohols and amines to convert them to trimethylsilyl ethers and trimethylsilyl amines; it can also react with carboxylic acid and water). Chemical tests using 2,4-dinitrophenyl hydrazine and Tollens reagent both resulted to negative results. The IR spectrum for the compound (in KBr disk) is shown below. L00 S000 2000 1000 KAVENUNB ERI Propose the structure for the compound that best fits these data. Illustrate the orbitals involved for the electronic transitions for this compound, consider different types of chromophore.

An organic compound (with an index of hydrogen deficiency of 1), containing only carbon, hydrogen, and oxygen was burned in excess oxygen. When 12.915 g of the organic compound is burned, this produced 18.942 g carbon dioxide and 7.749 g of water. The organic compound was reacted with 3 moles of trimethylsilyl chloride (TMSCI) as protecting agent (used to protect alcohols and amines to convert them to trimethylsilyl ethers and trimethylsilyl amines; it can also react with carboxylic acid and water). Chemical tests using 2,4-dinitrophenyl hydrazine and Tollens reagent both resulted to negative results. The IR spectrum for the compound (in KBr disk) is shown below. L00 S000 2000 1000 KAVENUNB ERI Propose the structure for the compound that best fits these data. Illustrate the orbitals involved for the electronic transitions for this compound, consider different types of chromophore.

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

Hydrolysis of a compound B(C2H4Cl2)was carried out by refluxing with excess potassium hydroxide solution. The resulting solution was acidified with dilute nitric acid and excess silver nitrate added to precipitate the chloride ions as silver chloride,0.718g of silver chloride was formed from 0.805g of B. (a) Calculate the number of chlorine atoms present in each molecule of B which are liberated by hydrolysis. (b) Suggest an explanation for the result obtained in (a) (c) Give a possible structure for B
What is the mole ratio for O2 gas to water for the balanced equation for the complete combustion of butane. 2C4H10(g)+ 13O2(g)-> 10H2O(g) + 8CO2(g)
6. Suppose a pond's water contains 10.0 mg/L of some algae, which can be represented by the chemical formula C6H₁5O6N. Using the following reactions: C6H1506N +60₂6CO2 + 6H₂O + NH3 NH3 + 202 → NO3 + H+ + H₂O Find the theoretical nitrogenous oxygen demand (NBOD) (mg/L) Atomic mass: C=12 H=1 O=16 N=14
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.
0.94g of salicylic acid was reacted with excess acetic anhydride in the presence of concentrated phosphoric acid (catalyst) to yield 0.80g of acetyl salicylic acid (see below). Determine the percent yield of acetylsalicylic acid. Hint: Percent yield = actual yield/theortical yield * 100% OH O OH Salicylic acid Chemical Formula: C7H6O3 Molecular Weight: 138.12 mp 159 °C 유 + H3C O CH3 acetic anhydride Chemical Formula: C₂H6O3 Molecular Weight: 102.09 bp 140 °C H₂PO4 H₂C 요 OH Acetylsalicylic acid Chemical Formula: CgH8O4 Molecular Weight: 180.16 mp 128-137 °C
The reaction for the oxidation of NH3 is given as: 4 NH3 + 5 024 NO + 6H₂O Under certain conditions the reaction will proceed at 29.8% yield of NO. How many grams of NH3 must be used to react with excess oxygen to yield 70.5 g of NO? Hint: 70.5 g of NO is the actual yield. 21.0 134 237 2.37 None of these responses apply.
The reaction 3Ox(g) + M(g) ⇋ 4N(g) has Kc = 67.10 Calculate Kc for the reaction: 2N(g) ⇋ 0.5 M(g) + 1.5 Ox(g)
Given (8.79x10^6) moles of glucose, C6H12O6, calculate the mole of carbon dioxide, CO2, formed upon complete oxidation of the glucose. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O Express your answer in three significant digits as moles. Note: Your answer is assumed to be reduced to the highest power possible.
Having one mole of carbon suboxide (C2O3) means that you have