Organic Chemistry Questions

A chemistry student must write down in her lab notebook the concentration of a solution of sodium hydroxide. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: The label on the graduated cylinder says: empty weight: 8.5 g She put some solid sodium hydroxide into the graduated cylinder and weighed it. With the sodium hydroxide added, the cylinder weighed 83.15 g. She added water to the graduated cylinder and dissolved the sodium hydroxide completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 97.85 mL. What concentration should the student write down in her lab notebook?

Consider the structure of hex-3-ene. Which of the following statements describes this compound? The heat of combustion of the cis isomer is lower than that of the trans isomer. The cis isomer is more stable than the trans isomer. Conversion of the trans isomer to the cis isomer would have a negative AG. The cis isomer acts as a Lewis base while the trans isomer acts as a Lewis acid. Stereoisomerism is not possible for this substance.

Draw structures using wedges and hashed lines where necessary which fit the following descriptions: (16 points) (a) one isomer of 1,2,4-trimethylcyclohexane that is chiral: (b) two enantiomers of 2,3-butanediol as their line-angle formulas:

Which of the following molecules would exhibit cis-trans isomerism? 3-ethyl-5-methyloct-3-ene pent-2-ene but-1-ene 2,3-dimethylbut-2-ene Both pent-2-ene and 3-ethyl-5-methyl-3-ene

Thailanstatin A is a natural product that was isolated from Thailandensis burkholderia MSMB43, and has been studied for use as an anticancer agent. Answer the following questions related to this molecule. a. Circle and label all functional groups (Be sure to label any amines or alcohols as primary, secondary, or tertiary). b. Clearly label one primary carbon, one secondary carbon, and one tertiary carbon.

Provide the expected product for the reaction of each of the following alkenes with H₂SO4 and H₂O. If you expect a racemic mixture or an equimolar mixture of diastereomers, draw both stereoisomers. Draw the molecule(s) on the canvas by choosing buttons from the Tools (for bonds and charges), Atoms, and Templates toolbars. Show the appropriate stereochemistry by choosing the dashed or wedged buttons and then clicking a bond on the canvas.

You will require the following molecule diagrams for your individual assignment on Blackboard: Question: Functional groups Classify each of the following molecules according to it's functional group.

Consider the following cyclohexane a) Draw a chair conformation for the cyclohexane derivative above showing equatorial and axial positions at the carbon atoms bearing the substituents. b) Draw the flipped chair conformation showing axial and equatorial position at the carbon atoms that bear the substituents. Determine which structure is more stable (8a or 8b)? Describe and give your reasons.

A cylindrical piece weighs 20 gram. When it is dropped into a graduated cylinder, the volume of water rises from 50.0 ml to 55.5 ml. What is the volume used to find density? a. 105.5 ml b. 55.5 ml c. 50 ml d. 5.5 ml

What is the index of hydrogen deficiency for each of the following molecular formulas? C6H8O2 Express your answer as an integer.

Given the name, draw the structure of the following compounds. cis-6,7-dimethylcyclohepta-1,4-diene Draw the molecule on the canvas by choosing buttons from the Tools (for bonds and charges), Atoms, and Templates toolbars. Show the appropriate stereochemistry by choosing the dashed or wedged buttons and then clicking a bond on the canvas.

Compare 1-butene to butane. Which of the following would definitely be different between these two species? boiling point free bond rotation Both bond rotation and IHD. water solubility IHD

Rank the following carbocations from most stable to least stable. (Carbocations, like radicals, are electron deficient.)

If one wanted to convert 1-ethylcyclohexene to ethylcyclohexane, this could be accomplished by using which of the following reagents? HBr, H₂O2 H₂SO4, H₂O HBr H₂ and Pt catalyst.

Predict the product(s) you would get when the following alkene reacts with H₂SO4 and H₂O: If you expect a racemic mixture, draw both enantiomers.

(C3H8, 44.1 g/mol) is a common fuel for barbeque grills and camp stoves and is sold in canisters. The combustion reaction of propane is shown in the equation below. In an experiment, 16 ounces of liquid propane was combusted in the presence of excess oxygen, and the resulting carbon dioxide (465.8 g) was captured. What is the percent yield for carbon dioxide in this experiment? (Density of C3H8 is 0.493 g/mL)

Which of the following could probably not be produced by electrophilic addition of an alkene? 2-bromo-4-methylpentane 2-bromo-2-methylpentane 1-bromohexane 2-bromopentane

Calculate the percent yield in the photosynthesis reaction by which carbon dioxide is converted to sugar if 7.03 g of carbon dioxide yields 3.92 g of C6H12O6. The equation is 6 CO₂ + 6 H₂O → C6H12O6 +6 02.

Ammonia can be produced by reacting nitrogen gas with hydrogen gas. N2 + 3H2 → 2NH3 If 1.40 g of nitrogen and 0.400 g of hydrogen are used, which reactant is in excess and how much remains? How much ammonia can be produced?

The first step in the Ostwald process for manufacturing nitric acid is the reaction between ammonia and oxygen described by the equation 4NH3 +502 4NO + 6H₂O. Use this equation to answer the following three questions. 19. How many moles of ammonia will react with 95.3 moles of oxygen? 20. How many moles of nitrogen monoxide will result from the reaction of 2.89 moles of ammonia? 21. If 3.35 moles of water is produced, how many moles of nitrogen monoxide will also be produced? 22. Magnesium hydroxide is formed from the reaction of magnesium oxide and water. How many moles of magnesium oxide are needed to form 0.884 moles of magnesium hydroxide, when the oxide is added to excess water?

Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of CO₂ according to the following combustion reaction: 2 C4H10(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)

Which of these sentences with can or able to is grammatically correct? A) I not able to swim very fast. B) I can't swim very fast. C) I will be able swim very fast. D) I cannot to swim very fast.

Which of these sentences about asking or giving advice correct (page 193)? A) You should not to pack your suitcase now. B) You should not be packing your suitcase now. C) You should not packing your suitcase now. D) You should not packed your suitcase now.

How many moles of Care formed upon complete reaction of 2 mol of B according to the generic chemical reaction: A + 2 B-C

After reading/listening to "The Family Life of Lowland Gorillas" on page 4, doing the exercises, ad reading grammar explanations, answer these questions. When do we usually use Simple Present tense? A) For simple actions B) To describe routines and habits C) To present facts and general truths D) To describe temporary situations E) B ad C

Determine the number of grams of HCI that can react with 0.750 g of Al(OH)3 according to the following reaction Al(OH)3(s) + 3 HCl(aq) → AICI3(aq) + 3 HO(aq)

1. Draw structures for the products of the Diels-Alder reactions between a) 1,3-cyclopentadiene and maleic anhydride. b) 1,3-butadiene and trans-CH₂-CH=CH-CH=0. c) anthracene and HO₂C-C=C-CO₂H.

Use the Internet or another resource to find out how the size of an atom compares with the size of its nucleus. Is the diameter of an atom 10 times, 1,000 times, or 100,000 times the diameter of the nucleus?

What does bolded text mean in the sentence on page 176 "They often had to hold their breath." A) it was necessary to do it B) they were ordered to do it C) they were not allowed to do it D) they were expected to do it

Limestone stalactites and stalagmites are formed in caves by the ollowing reaction: Ca²+ (aq) + 2HCO3(aq) → CaCO3(s) + CO2(g) + H₂O(1) f 1 mol of CaCO3 forms at 298 K under 1 atm pressure, the reaction performs 2.49 kJ of P-V work, pushing back the atmosphere as the gaseous CO₂ forms. At the same time, 38.85 J of heat is absorbed from the environment. What is the value of AH for this reaction? Express your answer using four significant figures

Convert a pressure of 1379 torr to atm.

In the reaction shown below, how much of 1.15 M solution of AgNO3 is needed to completely react with 0.421 mol of magnesium chloride according to the equation: MgCl₂(aq) + 2 AgNO3(aq) → Mg(NO3)2(aq) + 2 AgCl(s) 0.968 L 0.484 L 36.6 mL 0.366 L 0.732 L

The addition of chromic acid or chromate is a qualitative test for alcohols as the reaction causes a color change. However, not all alcohols react with chromic acid or chromate. Determine whether the named alcohol will react with chromic acid or chromate to cause a color change. 3-hexanol Choose... 3-ethyl-3-pentanol Choose.... 1-butanol Choose... 2-pentanol Choose...

Calculate the mass of water produced when 6.51 g of butane reacts with excess oxygen.

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory. At times it can be easier to chemically prepare occasionally used gases. For example, nitrogen monoxide, NO(g), can be prepared in the lab using the following chemical reaction: 3Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H₂O(1) If 5.0 g of copper metal was added to an aqueous solution containing 2.5 moles of HNO3, how many moles of NO(g) would be produced, assuming a 100% yield? 0.042 mole NO 0.052 mole NO 0.062 mole NO

Carbon tetrachloride was widely used for many years as a solvent until its harmful properties became well established. Carbon tetrachloride may be prepared by the reaction of natural gas (methane, CH₂) and elemental chlorine gas in the presence of ultraviolet light. Choose the unbalanced chemical equation for this process. CH₂(g) + HI(g) → CCL (1) CHI(g) + O₂(g) → CCL (1) + HCl(g) CH. (g) → CCL (1) + HCl(g) CH₁ (9) + Cl₂(g) → CCL (1) + HCl(g)

Complete the sentences to explain the kind of ring structure a Haworth structure of fructose has. Match the numbers in the left column to the appropriate blanks in the sentences on the right. In the ring structure of fructose, there are atom(s). carbon atom(s) and The ring is a result of the formation of a hemiacetal where the hydroxyl group on carbon reacts with the ketone group on carbon

Balance the following chemical equation: RbO₂ (s) + H₂O(l) → RbOH(aq) + O₂(g) + H₂O₂ (aq) 3RbO₂ (s) + H₂O(l) → RbOH(aq) +202 (9) + H₂O2 (aq) 4RbO₂ (s) + 6H2₂O(l) → 4RbOH(aq) + O₂(g) + 4H₂O₂ (aq) RbO₂ (s) + H₂O(l) → RbOH(aq) + O2(g) + H₂O₂(aq) RbO₂ (s) + 2H₂O(1)→ 5RbOH(aq) + O2(g) + H₂O₂ (aq) b Balance the following chemical equation: MgO(s) + HNO3(aq) → Mg(NO3)2 (aq) + H₂O(l) 5MgO(s) + 3HNO3(aq) → 5Mg(NO3)2 (aq) + H₂O(1) 2MgO(s) + 2HNO3(aq) → Mg(NO3)2 (aq) + 3H₂O(1) MgO(s) + HNO3(aq) → Mg(NO3)2 (aq) + H₂O(1) MgO(s) + 2HNO3(aq) → Mg(NO3)2 (aq) + H₂O(l) C Balance the following chemical equation: C3H8 (g) + O2(g) → CO₂(g) + H₂O(g) C3Hs (g) + 802(g) → 3CO₂(g) + H₂O(g) C3H8 (g) +502 (g) → 3CO2(g) + 4H₂O(g) C3Hs (9) + O2(g) → CO₂(g) + H₂O(g) C3Hs (g) + 802(g) → 3CO2(g) + 2H₂O(g)

Write the balanced equation for this reaction (in lowest multiple integers).

Acetylene gas (C₂H₂) is often used by plumbers, welders, and glass blowers because it burns in oxygen with an intensely hot flame. The products of the combustion of acetylene are carbon dioxide and water vapor. Choose the unbalanced chemical equation for this process. C₂H₂(g) + H₂O(g) → CO₂(g) + O2(g) C₂H₂(g) + N₂(g) → CO₂(g) + H₂O(g) C₂H₂(g) + O₂(g) → CO₂(g) + H₂O(g) C₂H₂(g) → CO₂(g) + H₂O(g) + O2(g)

arbon tetrachloride was widely used for many years as a solvent until its harmful properties became well established, Carbon tetrachloride may be prepared by the reaction of natural gas (methane, CH,) and elemental lorine gas in the presence of ultraviolet light. Choose the unbalanced chemical equation for this process. CH₂(g) + HCl(g) → CCL (1) CH (9) + O2(g) → CCL (1) + HCl(g) CH (9)→ CCL (1) + HCl(g). CHI(g) + Cl₂(g) → CCL (1) + HCl(g)

Solid iron(II) oxide reacts with oxygen gas to produce solid iron(III) oxide. Balance the equation for this reaction (in lowest multiple integers). What are the formulas for the reactants and product?

Rubidium oxide is sometimes very challenging to store in the chemistry laboratory. This compound reacts with moisture in the air and is converted to rubidium hydroxide. If a bottle of rubidium oxide is left on the shelf too long, it gradually absorbs moisture from the humidity in the laboratory. Eventually, the bottle cracks and spills the rubidium hydroxide that has been produced. Choose the unbalanced chemical equation for this process. RbOH(s)→ Rb₂O(s) + H₂O(g) Rb₂O(s)→ RbOH(s) + H₂O(g) RbOH(s) + H₂O(g) → Rb₂O(s) Rb₂O(s) + H₂O(g) → RbOH(s)

The element tin often occurs in nature as the oxide SnO₂. To produce pure tin metal from this sort of tin ore, the ore usually is heated with coal (carbon). This produces pure molten tin, with the carbon being removed from the reaction system as the gaseous by-product carbon monoxide. Choose the unbalanced chemical equation for this process. Previous Page 4 of 12 SnO₂ (s) + O₂(g) + C(s) → Sn(1) + C(g) SnO₂ (s) + C(s) → Sn(l) + CO₂(g) SnO₂ (s) + CO(g) → Sn(1) + C(s) SnO₂ (s) + C(s) → Sn(1) + CO(g)

When elemental phosphorus, P4, burns in oxygen gas, it produces an intensely bright light, a great deal of heat, and massive clouds of white, solid phosphorus(V) oxide (P₂O5) product. Given these properties, it is not surprising that phosphorus has been used to manufacture incendiary bombs for warfare. Choose the unbalanced equation for the reaction of phosphorus with oxygen gas to produce phosphorus(V) oxide. P₂O5 (s)→ P4(s) + O2(g) P₂O5 (8) + P4 (8) → O2(g) P4(s) + O2(g) → P2O5 (8) P4(s) → P2O5 (8) + O2(g)

Nitrous oxide gas (systematic name: dinitrogen monoxide) is used by some dental practitioners as an anesthetic. Nitrous oxide (and water vapor as a by-product) can be produced in small quantities in the laboratory by carefully heating of ammonium nitrate. Choose the unbalanced chemical equation for this reaction. NH4NO3 (8) + H₂O(s) → N₂O(g) NH4NO3(s) + O2(g) → N₂O(g) NH4NO3(s) + N₂(g) → N₂O(g) + H₂O(g) NH4NO3(s) → N₂O(g) + H₂O(g)

Add one or more curved arrows to show the movement of electrons in the reaction: To draw the arrows, select More in the drawing menu, then select the appropriate curved arrow. Click on a bond or electron to start a curved arrow. Do not start from an atom. Use the select tool to move the arrow head and tail to the desired placement. The curved arrow changes from red to black when appropriately placed.

In addition to your regular PreLab: 1. Look up the boiling points for 2-methylcyclohexanol methylcyclohexene and 3-methylcyclohexene. (cis/trans mixture), 1- 2. Calculate the volume needed to acquire 0.1 mole of 2-methylcyclohexanol. You'll need to figure out the molar mass. The density is 0.94 g/mL.

Barium chloride is used in the manufacturing of pigments, and may be synthesized by direct combination of its constituent elements. Choose the unbalanced chemical equation for this process. BaO(aq)+Cl(g) → BaCl,(s) +0,(g) Ba(s) + Cl₂(g) → BaCl₂ (s) BaCl(s) + Cl₂ (9)→ BaCl₂ (8) Ba(s) + O₂(g) → BaCl₂ (s)

Pure silicon, which is needed in the manufacturing of electronic components, may be prepared by heating silicon dioxide (sand) with carbon at high temperatures, releasing carbon monoxide gas. Choose the unbalanced chemical equation for this process. SiO₂ (s) + C(s) → Si(s) + CO(g) SiO2 (s) + CO(s) → Si(s) + CO₂(g) SiO2 (s) + CO2 (s) → Si(s) + CO(g) + O₂(g) SiO2 (s) + C(s) + O₂(g) → SiO₂ (s) + CO(g)