The equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N₂O₄(g) ⇌ 2NO₂(g)

Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur?

equilibrium, left, right? P_NO2 = 0.154 atm, P_N2O4 = 0.148 atm

equilibrium, left, right? P_NO2 = 0.210 atm, P_N2O4 = 0.138 atm

equilibrium, left, right ? P_NO2 = 0.149 atm, P_N2O4 = 0.05 atm

equilibrium, left, right? P_NO2 = 0.087 atm, P_N2O4 = 0.13 atm

equilibrium, left, right? P_NO2 = 0.068 atm, P_N2O4 = 0.058 atm

1. The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can be produced by combining 67.1 g of each reactant?

2. In the following reaction, how many grams of sodium sulfate, Na2SO4, will be produced from 80.7 g of sodium hydroxide, NaOH?

This problem is a long one, but fairly conceptual in nature.

a. For each of the following salts, write the reaction that occurs when it dissociates in water: NaCl(s), NaCN(s), KClO2(s), NH4NO3(s), KBr(aq), NaF(s).

b. Consider each of the reactions that you wrote above, and identify the aqueous ions that *could* be proton donors (acids) or proton acceptors (bases). Briefly *explain how you decided which ions to choose*.

c. For each of the acids and bases that you identified in part b, write the chemical reaction it can undergo in aqueous solution (its reaction with water).

d. Are there any reactions that you have written above that you anticipate will occur to such an extent that the pH of the solution will be affected? As part of your answer, be sure to explain how you decided.

e. Assume that in each case, above, 0.01 mol of the salt was dissolved in enough water at 25 deg Celsius to make 1.0L of solution. In each case, what additional information would you need in order to calculate the pH? If there are cases where no additional information is required, be sure to state that as well.

f. Say you take 0.01 mol of NH4CN and dissolve it in enough water at 25 deg Celsius to make 1.0L of solution. Using chemical reactions and words, explain how you would go about determining what effect this salt will have the pH of the solution. Be sure to list any additional information you would need to arrive at an answer.

Following are the post-lab questions for the experiment: Magnetic Behavior and Electron Configuration of Compounds Version

1. Chromium, Cr, has 24 electrons. Write out the entire electron configuration for chromium using spdf notation.

2. How many unpaired electrons would you expect for chromium in [Cr(H2O)6] 3+? Is this a paramagnetic or diamagnetic material?

3. Cobalt, Co, has 27 electrons. Write out the entire electron configuration for cobalt using spdf notation.

4. How many unpaired electrons would you expect for manganese in KMnO4? Is this a paramagnetic or diamagnetic material?

5. This same experiment is performed on the international space station. What is the primary issue with performing this experiment in the absence of gravity? Design an experiment to compensate for this. As always, you do have duct tape.

PART A:

Calculate pH for strong base solution: 7.4×10⁻² M KOH.

Express your answer using two decimal places.

PART B:

Calculate pH for strong base solution: 1.065 g of KOH in 510.0 mL of solution.

Express your answer using four decimal places

PART C:

Calculate pH for strong base solution: 15.0 mL of 1.90×10⁻² M Ca(OH)2 diluted to 510.0 mL.

Express your answer using three decimal places.

I am trying to find the percent yield of my final product in a Diels-Alder reaction. The weight of our final endo product (Cis-norborene-5,6-endo-dicarboxylic anhydride) was 5.025 grams. When performing the reaction, we used 2.5 grams of maleic anhydride and 2.5mL of cyclopentadine. Assume average molecular weight for the reagents.

How would you go about finding the %RAD for a titration experiment?

What is the mass per repeating unit of PET (in g/mol)? explain why this number should be used ffor determning limiting reagent and yield and not the actual molecular weight of the polymer (which is >> 10,000 g/mol). I know that the mass per repeating unit of PET is 192 g/mol.

Please answer the following question:
Window glass is colorless in the usual thickness used, but appears slightly green when viewed from the edge due to small amounts of Fe³⁺ . Why is this so?

How do you prepare 25 ml of 8.5 mM NaCl from a 20% NaCl stock? (Hint: convert 20% to g/ml then to molar)

For each pair of substances determine which has the higher entropy per mole of substance.

a. H2O (s) at 200 K or H2O(s) at 298 K.

b. H2(g) at 298 K, 2.0 atm or H2(g) at 298 K, 1.0 atm.

c. H2(g) at 298 K, 5.0 L or H2(g) at 298 K, 1.0 L

Accoring to the equation: As_sO₃ + 3C = 3CO +2As

the reaction of 1gmol of As_sO_{3 with carbon will result in the formation of:}

_{A. 1 gmol of CO}

_{B. 1 gmol of As}

_{C. 28 g of CO}

D. 150 g of As

A)Consider the following gases, all at STP: Ne, SF6, N2, CH4.

Which gas is most likely to depart from assumption 3 of the kinetic molecular theory (Attractive and repulsive forces between gas molecules are negligible.)?

Which one is closest to an ideal gas in its behavior?

Which one has the highest root-mean-square molecular speed?

Which one has the highest total molecular volume relative to the space occupied by the gas?

Which has the highest average kinetic molecular energy?

Which one would effuse more rapidly than N2?

B) A mixture of gases contains 0.75mol N2, 0.35mol O2, and 0.20mol CO2. The total pressure of the mixture is 1.57atm .

What is the partial pressure of O2?

What is the partial pressure of CO2?

C) What is the partial pressure in atm of O2 of this mixture if it is held in a 12.60?L vessel at 14?C? (O2 =.149mole)

What is the partial pressure in atm of N2 of this mixture if it is held in a 12.60?L vessel at 14?C? (N2= .241mole)

What is the partial pressure in atm of H2 of this mixture if it is held in a 12.60?L vessel at 14?C?(H2= .610mole)

Using the following equation (Debye-Huckel), find the coefficient of activity of the following:

a) Fe³⁺ with I = 0.062M answer should be 0.22

b) Ce⁴⁺I = 0.070M answer should be ≈ 0.08

c) Pb²⁺  I = 0.042M

Note: if you attempt this question please solve all parts (a,b and c) or else your answer will be rated as wrong/reported.

For the following reaction, KcKc = 255 at 1000 KK.
CO (g) + Cl2 (g) ⇌ COCl2 (g)CO (g) + Cl2 (g) ⇌ COCl2 (g)
A reaction mixture initially contains a COCO concentration of 0.1550 MM and a Cl2Cl2 concentration of 0.173 MM at 1000 KK.

a) What is the equilibrium concentration of COCO at 1000 KK?

b) What is the equilibrium concentration of Cl2Cl2 at 1000 KK?

c) What is the equilibrium concentration of COCl2COCl2 at 1000 KK?

please show work!