Organic Chemistry Answers

. What are the types of attractive forces that can exist between the molecules of each of the following? HI , F2 , H2O

2. Draw formulas showing the covalent and ionic bonds of the following two compounds? CH3ONa, NH4Cl

explain the following statement a) for diels alder reaction a diene must be able to adopt a cis geometry b) low molecular weight ozonides cannot isolated easily c) alkenes are readily hydroxylated

Explain Ceramic matrix nanocomposites

Applications of hybrid organic nanocomposites

Explain types of hybrid organic nanocomposites

What is hybrid organic nanocomposites

Draw the resonance structures of cyanate ion. Out of them which one is less important

as a resonance structure and why?

POLYER LAB  Chemistry 30

1. Use a graduated cylinder (or teaspoon)* to add 10 mL of tap water to a Dixie Cup. With a pen, mark the level of the water on the outside of the cup. Add an additional 10 mL of water to the cup and mark the water level. Repeat 2 times until a total of 40 mL has been added to the cup. Now dump out all the water. 2. Measure 10 mL of tap water into the Dixie cup and add 3-4 drops of food coloring. 3. Using the markings on the Dixie cup, add ~10 mL of Elmer’s white glue directly to the cup and mix (stir rod

or spoon) gently until the mixture has a uniform consistency. 4. Use a graduated cylinder (or 1⁄2 cup measuring cup) to measure 125mL of tap water in a beaker (larger plastic

container). an electronic balance, weigh boat (or wax paper) and a scoopula (or teaspoon), add 8.7 grams of Borax to the water. This is your saturated (6.5%) sodium tetraborate solution. solid is dissolved.

1.     The food we eat is degraded, or broken down, in our bodies to provide energy for growth and function. A general overall equation for this very complex process represents the degradation of glucose (C₆H₁₂O₆) to carbon dioxide (CO₂) and water (H₂O):

C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O

If 968 g of C₆H₁₂O₆ is consumed by a person over a certain period, what is the mass of CO₂ produced?                                                                                         

2.     Urea [(NH₂)₂CO] is prepared by reacting ammonia with carbon dioxide:

2NH₃(g) + CO₂(g) → (NH₂)₂CO(aq)+ H₂O(l)

In one process, 849.2 g of NH₃ are treated with 1223 g of CO₂.                       

(a) Which of the two reactants is the limiting reagent?

(b) Calculate the mass of (NH₂)₂CO formed.

 (c) How much excess reagent (in grams) is left at the end of the reaction?