Organic Chemistry Questions

Butane gas (C4H10) burns in oxygen gas to produce carbon dioxide gas and water vapor. Balance the equation for this reaction (in lowest multiple integers). To check if you balanced the equation correctly, make sure the number of each type of atom totals the same on both sides of the equation.

The illustration on the left represents a mixture of H₂ (light blue) molecules and I₂ (purple) molecules. If these were to react to form HI molecules, what is the maximum number of HI molecules that could form?

Methanol (methyl alcohol), CH3OH, is a very important industrial chemical. Formerly, methanol was prepared by heating wood to high temperatures in the absence of air. The complex compounds present in wood are degraded by this process into a charcoal residue and a volatile portion that is rich in methanol. Today, methanol is instead synthesized from carbon monoxide and elemental hydrogen. Choose the balanced chemical equation for this latter process. 3H₂(g) + 2CO2(g) → 2CH3OH(g) 2H₂(g) + CO(g) → CH3OH(9) 2CH3OH(g) → 3H₂(g) + 2C(g) CH₂OH(g) → H₂(g) + 3CO(g)

A common demonstration in chemistry courses involves adding a tiny speck of manganese (IV) oxide to a concentrated hydrogen peroxide, H₂O2, solution. Hydrogen peroxide is unstable, and it decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese (IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Choose the balanced equation for the decomposition reaction of hydrogen peroxide. H₂O₂ (aq) → 3H₂O(g) + O₂(g) 2H₂O₂ (aq) → 3H₂O(g) +20₂ (9) 2H₂O₂ (aq) → 2H₂O(g) + O₂(g) H,Oz(aq) → H_O(g)+Oz(g)

For each pair, choose the combination of nucleophile and solvent that would give the faster SN2 reaction with ethyl iodide. Explain why. a. NaOCH₂CH3 in ethanol or NaOCH₂CH3 in DMSO. b. NaOCH₂CH3 in acetic acid or NaOCH₂CH3 in DMF.

What is the name of the following compound based on the Lewis-Dot structure? (SC.912.P.8.7) a. sulfur oxide b. sulfur trioxide c. monosulfur oxide d. monosulfide trioxide

Calculate the iso-electric points (pl) for the following AA's (compare the results): 1. Phenyl alanine, pK1 = 2.2 and pK2 = 9.31 2. Aspartic acid, pK1 = 1.99, pK2 = 3.90 and pK3 = 9.90 3. Histidine, pK1 = 1.80, pK2 = 6.04 and pK3 = 9.33

A student collected 88.0 mL of carbon dioxide at 28.00C and 730 torr. What volume of carbon dioxide would the student have at 28.00C and 760 torr?

Consider the following hypothetical acid-base reaction HOH + Y 2 OH + HY for which the transition state is represented as the reaction rate depends only on the concentration of HOH. the reaction is overall first order. the reaction is first order with respect to water. R = K[HOH][Y] Both C and D

A gas cylinder contains exactly 15 moles of oxygen gas (O₂). How many molecules of oxygen are in the cylinder? 4.01 x 1022 molecules 6.02 x 1023 molecules 9.03 x 1024 molecules 2.89 x 1026 molecules

Benzene has a 6-carbon ring, with alternating single and double bonds. Consider a benzene molecule in which a hydrogen atom is replaced by an aldehyde functional group. Draw the molecule produced.

Amino acids are the building blocks for proteins. Each amino acid contains an amine group (-NH), a carboxyl group (-COOH), and an R group called a side chain. These are all bonded to a carbon called the alpha carbon. The R groups are different for each amino acid. In addition to the name of the amino acid, each one has a three-character and a one- character abbreviation. Which choice correctly pairs the name of the amino acid with its three-character abbreviation?

The pure, natural enantiomer of (-)-menthol, has an specific rotation [a]20 = -50° (Formula: (A-B)/(A+B) = ee = ap20/[a]020 - show work!) a) What is the ee of a mixture of 1.50 g (+)-menthol and 3.50 g (-)-menthol? b) What is the rotation co2 of this mixture under standard conditions?

Given the following reaction below, how many moles of H 20 can be formed from 0.03352 moles of C 6H 14? 12 CO 2 (g) + 14 H 20 (g) 2 C 6H 14 (g) + 19 O 2 (g) 0.004789 mol 2.315 mol 0.3185 mol 4.261 mol 0.2347 mol

What is the molecular formula of oxybenzone?

A 0.5881 g sample of impure magnesium hydroxide is dissolved in 105.0 mL of 0.2047 M HCl solution. The excess acid then needs 19.85 mL of 0.1050 M NaOH for neutralization. Calculate the percent by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

The rate of a given reaction will increase as the orientation specificity decreases. rate constant increases. activation energy decreases. temperature increases. All of the factors listed.

A sample of an unknown contains 30.4% nitrogen and 69.6% oxygen. What is the empirical formula for this compound?

A medical lab is testing a new anticancer drug on cancer cells. The drug stock solution concentration is 1.5 x 10-9M, and 4.00 mL of this solution will be delivered to a dish containing 2.0 x 105 cancer cells in 5.00 mL of aqueous fluid. What is the ratio of drug molecules to the number of cancer cells in the dish?

Tartaric acid, H₂ C4 H4 O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 21.65 mL of 0.2500 M NaOH solution to titrate both acidic protons in 40.00 mL of the tartaric acid solution. Write a balanced net ionic equation for the neutralization reaction.

Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are called alloys. There is a range of compositions over which the solution is considered a bronze. Bronzes are stronger and harder than either copper or tin alone. A 200.0-g sample of a certain bronze is 90.0% copper by mass and 10.0% tin. Which metal can be called the solvent, and which the solute? Tin is the solvent and copper is the solute. Copper is the solvent and tin is the solute. Copper is both the solvent and the solute. Tin is both the solvent and the solute.

Formic acid, HCOOH, is a weak electrolyte. What solute particles are present in an aqueous solution of HCOOH? Weak electrolytes such as formic acid (HCOOH) will be present mostly in solution in its neutral form, with only a small fraction dissociated into ions. For example, in a solution of acetic acid (CH3 COOH), only a small fraction is dissociated into H+ and CH3COO ions. Enter the chemical equation for the ionization of HCOOH.

Tartaric acid, H₂ C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 21.65 mL of 0.2500 M NaOH solution to titrate both acidic protons in 40.00 mL of the tartaric acid solution. Write a balanced net ionic equation for the neutralization reaction.

An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of NaCl of the same concentration. Which of the following substances could the unknown be? KOH NH3 HNO3 KCIO₂ H3PO3 CH3COCH3

C6H12O6 is an organic compound. Calculate its molar mass to 2 decimal spaces.

A solution is made by mixing 13.0 g of Sr(OH)2 and 35.0 mL of 0.180 M HNO3. Calculate the concentration of NO3 ion remaining in solution.

Which orbital notation correctly represents the outermost principal energy level of a nitrogen atom in the ground state?

Predict the product(s) of the following reaction. How many products are formed? Name the product with the most carbons overall. What is the molecular formula of the product with the most carbons overall (in alphabetical order).

On each chair structure identify the relationship of the substituents as cis or trans? I = trans; II = trans l =cis; 11 = cis I = trans; 11 = cis I=cis; II trans not possible to tell while in a chair structure

Identify the correct chair conformations of the following compound and then indicate which one is more stable. I and II are correct chair structures and I is most stable I and II are correct chair structures and II is most stable I and III are correct chair structures and III is most stable II and III are correct chair structures and II is most stable II and III are correct chair structures and III is most stable

A student performing the experiment "Titration of Acetic Acid in Vinegar" got mixed up where to put the solutions. He put the vinegar in the titrator, and the measured amount of NaOH solution in the beaker. He added the phenolphthalein in the beaker containing the NaOH. If he runs the titration with this set-up, what do you expect to happen to his experiment? The solution in the beaker will initially be colorless, and the color changes from colorless to pink at the equivalence point. The experiment will not work because it is not possible to predict the color change at the equivalence point. The experiment will not work because there will be no color change at the equivalence point. The solution in the beaker will initially be pink, and the color changes from pink to colorless at the equivalence point.

A solution of NH2Br is rapidly made acidic and the [NH2Br] is followed as the reaction proceeds to form NHBr2. A plot of 1/[NH2Br] on the Y axis and time on the X axis is seen to be linear. a. The reaction is first order with respecct to NH₂Br. b. The reaction is zero order with respect to NH₂Br. c. The reaction is second order with respect to NH₂Br d. The reaction order cannot be determined in this manner. e. The [NHBr2] must be followed to determine the order in [NH2Br].

Calculate the energy (J) change associated with an electron transition from n=1 to n = 5 in a Bohr hydrogen atom. Specify if the energy is released or absorbed by the electron during this transition.

When the ideal gas law is arranged as shown below, what property of the gas is being solved for (represented by the X)? Moles Pressure Temperature Volume

How do the calculations look like to prepare 210.0 ml of 0.25 M nitric acid solution from a 0.60 M nitric acid solution. a) How much of the 0.60 M nitric solution is needed? b) How much water will you need to add to make that solution?

How many molecules of carbon dioxide will be formed if 6.71 g of propane is burned in the following reaction? C₂H₂(g) +50₂(g) →3CO₂(g) + 4H₂O(g) 1.21 x 1025 molecules 9.16 x 1022 molecules 3.67 x 1023 molecules 2.75 x 1023 molecules 4.58 x 1023 molecules

At the same temperature what weight of glucose in grams when dissolved in 100 g of water will produce the same lowering of vapour pressure as one gram of urea dissolved in 50 g of water. [Consider solutions to be highly diluted].

The presence of [Select] on the central atom is an indicator that the molecule is polar, if there are 3 or 4 electron regions. Two shapes that are always polar are bent and [Select]

For this assignment, the target compound that you should synthesize is chloro-cyclohexane. This is a substitution reaction. List the starting materials, solvent, reagent, and products formed: cyclohexanol, Hydrochloric acid, diethyl ether, Chlorocyclohexane, H20 Is this a substitution or an elimination reaction? Substitution reaction What is the leaving group in this reaction? H2O What is the nucleophile in this reaction?

Carbon-hydrogen bonds exhibit a range of different chemical reactivity that depends on molecular structure. Classify the C-H bonds at the carbons labeled a-c in the structure below. Possible classifications are: primary, secondary, & tertiary or none if there are no hydrogens at the labeled carbon.

Draw the molecule on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Advanced Template toolbars. The single bond is active by default.

The transformation above can be performed with some reagent or combination of the reagents listed below. Give the necessary reagent(s) in the correct order, as a string of letters (without spaces or punctuation, such as "EBF"). If there is more than one correct solution, provide just one answer.

Give the formula and name for the ionic compound formed from the combination of the indicated metal and carbonate, CO3 , a polyatomic ion. Express your answer as a chemical formula. formula: Spell out the full name of the compound.

CH3CH2CH2CH=CH2 Draw the molecule on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Advanced Template toolbars. The single bond is active by default.

Draw two constitutional isomers that share the molecular formula C₂H5N. Your structures will have the same molecular formula but will have different connectivities. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. • Separate structures with + signs from the drop-down menu.

A 0.698 mol sample of Xe gas is confined in a 17.4 liter container at 30.6 °C. If the temperature of the gas sample is decreased to 11.3 °C, holding the volume constant, the pressure will decrease because: Choose all that apply. With lower average speeds, on average the molecules hit the walls of the container with less force. At lower temperatures molecules have lower average speeds. As the number of molecule-wall collisions increases, the force per collision decreases. With higher average speeds, the molecules hit the walls of the container more often. None of the Above

A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat capacity of the metal.

A gas sample has a pressure of 747 mmHg when the temperature is 26 °C. Part A What is the final temperature, in degrees Celsius, when the pressure is 780 mmHg, with no change in the volume or amount of gas? Express your answer to two significant figures and include the appropriate units.

Draw a structural formula for the following alkene: cis-2-methyl-3-hexene ▪ Consider E/Z stereochemistry of alkenes. ▪ Do not show stereochemistry in other cases. ▪ You do not have to explicitly draw H atoms.

If you isolated 0. 650 g of nitroacetanilide (this is your actual yield) but your theoretical yield was 0.755 g, what is your percent yield? Hint: The equation to calculate your percent yield is shown below. % yield = actual yield / theoretical yield x 100% 86.1% 1.16% 0.861% 116%