Solution Investigation Question: What are some of the key characteristics of unknown sample of an aqueous solution containing an ionic compound?

Specific questions: 1. Given that the cation is from Group 1A, what is the identity of the group 1A metal ion in your solution?

2. Given that the ionic compound contains either chloride or hydroxide, how can you determine which? (Two pieces of evidence are required and one must be related to solubility rules)

3. What is the concentration of your solution? (Your unknown sample is known to be about 1 M, but you need to determine the concentration to 3 significant figures using titration. You should plan ahead so that you know approximately what volume of your sample you will need in order to use approximately 25 mL of 0.100 M sulfuric acid for the titration).

Calculate: grams of CO2 generated by a car for every kilometer I drive usings the quantiy of CO2 produced in part above (answer: 3088.2 g CO2) and kilometer distance traveled in part above (answer: 30.180 km/kg).

I'm having trouble converting CO2 generated to grams/km driven.

Illustrate and explain the importance of the urea cycle as it relates to nitrogen disposal. Explain the role of NAG in the regulation of CPSI activity and how this affects urea cycle function. Discuss how the urea cycle would be affected during a short-term fast (< 8 hr), long-term fast (> 24 hr), in response to a low (but adequate) protein diet, and in response to a high protein diet.

Write the balanced chemical reactions for the dissolution reactions AND the corresponding solubility product expressions for each of the following solids. Lastly, please calculate the solubility of each compound in pure water ignoring any acid-base properties.

a. Fe(OH)3

b. CuS

c. CaF2

All one question with a few different parts

Use the data to sketch the phase diagram for xenon (Xe) and then answer the questions that follow.

Normal boiling point: 165 K

Normal melting point: 161 K

Triple point: 152 K, .37 atm

Critical temperature: 290 K

Critical pressure: 57 atm

A. What phase is xenon at atmospheric conditions?

B. Is liquid xenon more or less dense than solid xenon? Use the diagram to justify your answer.

C. What is the appropriate maximum pressure of gas that can exist at -155 degrees Celsuis?

D. If a Xenon sample is heated at .2 atm, at what temperature will xenon melt? Explain.

E. Can xenon be liquid at room temperature if enough pressure is applied? Explain.

F. What is the minimum temperature at which the liquid phase can exist?

All part of one question, multiple steps

In the bromination reaction of a chalcone, trans-4-nitrochalcone reacts with Br2/CHCl3 to produce erythro-2,3-diBromo-3-(4-nitrophenyl)propiophenone. The product is a racemic mixture.

a) Draw the structure of the enantiomers you form and assign R & S to each of the stereocenters.

b) Will you see two spots on a TLC plate for your reaction products? Why or why not?

c) Draw the structures of the products that are not formed in the bromination reaction.

d) Is this bromination reaction stereoselective? Why or why not?

Plants produce sugar by photosynthesis. They absorb CO2, H2O and heat to produce sugar and oxygen. 
CO2  + H2O ? C6H12O6 + O2 (Unbalanced)
How much sugar will be produced if  8.0000 x10-3  ft3 CO2 gas (dCO2 = 1.98 kg/m3)  and 3.000 x 10-2 gallon water ( d= 0.9987 g /mL) is used. 

GaAs is zinc-blende with a = 0.56 nm, ε = 12.8, me* = 0.067me, and mh* = 0.2me.

(a) What is the exciton binding energy and radius?
(b) How many unit cells are contained within the n = 1 orbital?
(c) What is the highest temperature at which ground-state excitons are still observable?

why did my prof chose to right the stoichiometry of the combustion reaction for propane like this:

1/20 C3H8(g) + 1/4 O2(g) --> 3/20 CO2(g) + 1/5 H2O(l)

why did he write it in fractions, and its not because O2 is a diatomic.

he told does we have to get used to writing equations in fraction.

Ethane is chlorinated in a continuous reactor: C2H6 +Cl2 → C2H5Cl + HCl Some of the product monochloroethane is further chlorinated in an undesired side reaction: C2H5Cl +Cl2 → C2H4Cl2 + HCl

a. Take a basis of 100 mol of C2H5Cl produced. Assume that the feed contains only ethane and chlorine and that all of the chlorine is consumed. How many degrees of freedom remain (use atomic balances)?

b. The reactor is designed to yield a 19% conversion of ethane and a selectivity of 8 mol C2H5Cl / mol C2H4Cl2 with a negligible amount of chlorine in the product gas. Calculate the feed ratio (mol Cl2/mol C2H6).

Calculate the fractional yield (mol C2H5Cl produced / mol Cl2 consumed)

I did part a i am just confused about part b

Let 4 moles of methanol (liquid) combust in 3 moles of gaseous oxygen to form gaseous carbon dioxide and water vapor. Suppose this occurs in a chamber of fixed volume and fixed temperature. If the original pressure is 1.0 atm, what is the final pressure in the chamber. Express your answer in atm. Enter only a numerical value, do not enter units. Assume liquids take up negligible volume.

Consider the titration of 20.0 mL of 0.0800 M C5H5N (a weak base; Kb = 1.70e-09) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added:

(a) 0.0 mL pH =

(b) 4.0 mL pH =

(c) 8.0 mL pH =

(d) 12.0 mL pH =

(e) 16.0 mL pH =

(f) 22.4 mL pH =

Fe(NO3)₃. 9H₂O in 0.5M HNO₃ forms a colorless hexa-aquocomplex with the chemical formula {Fe(H2O)₆}³⁺ (aq).

This complex can then undergo an equilibrium reaction with potassium thiocynate (KSCN) to form a red complex with the chemical formula {Fe(H2O)5SCN}²⁺ (aq). In order to make this reaction occur, the two chemicals need to be mixed with 0.5M nitric acid. This equilibrium reaction is shown below:

{Fe(H₂O)₆}^₃₊ (aq) + SCN^-(aq) <--------> {Fe(H₂O)₅SCN}²⁺(aq) + H₂O (l)

a) When recording the absorbance values, what should be used as a blank slution and how show its data be treated?

b) K_eq is quoted to have a value of 250 at 20°C. When an initial potassium thiocynate concentration of 2x10^-4M was used, the red {Fe(H2O)₅SCN}²⁺ (aq) complex had an absorbance value of 0.5 . If the molar absorptivity coefficient of the red complex is 5400 cm-¹M^-1 and a 1 cm cuvette was used, calculate the equilibrium concentrations of [{Fe(H20)₆}³⁺(aq)]eq, [SCN^-]eq , [{Fe(H2O)₅SCN}²⁺_(aq)]_eq

c) Briefly describe the experiment you might conduct to determine if this reaction is endothermic or exothermic. What sort of results would lead you to conclude it was one or the other?

a) How many moles of Al₂(SO₄)₃ are required to make 45 mL of a 0.080 M Al₂(SO₄)₃ solution?
(Hint, molarity is moles per liter. You know the molarity. You are given the number of mL's, which can be converted to liters. Just set it up so the units cancel and you get "moles".)
_____________ moles Al₂(SO₄)₃

b) What is the molar mass of Al₂(SO₄)₃, to the nearest gram?
_____________ [grams/mole]

c) What mass of Al₂(SO₄)₃ is required to make 45 mL of a 0.080 M Al₂(SO₄)₃ solution?
(If you've got moles and molecular weight you can get to grams.)
______________ g Al₂(SO₄)₃

d) How many moles of aluminum ions are present in the solution?
(This is easy. You know how many moles of Al₂(SO₄)₃ there are from part a. Just think about how many aluminum ions there are per Al₂(SO₄)₃.)
______________ mol