A gaseous mixture of CO and CO2 has a density of 0.9967 g/L at 14.24°C and 490.1 mm Hg. What is the mass percent of CO?

A solution is made by mixing 15.5 g of Sr(OH)2 and 40.0 mL of 0.230 M HNO3.

Part A: Write a balanced equation for the reaction that occurs between the solutes.

Part B: Calculate the concentration of OH− ion remaining in solution.

Part C: Calculate the concentration of Sr2+ ion remaining in solution.

Part D: Calculate the concentration of NO−3 ion remaining in solution.

Part E: Is the resultant solution acidic or basic?

1) a) write balanced molecular and net ionic equations for the neutrilization of NaOH by KHP( mol. WT= 204.23). Khp is an abbreviation for potassium hydrogen phthalate, KHC8H4O4,a subtance of known high purity with one acid hydrogen as indicated by the formula.

b) if 2.8 g of 204.23 KHP is dissolved in water and titrated with 40 ml of NaOH to the phenolphthalein endpoint, what is the molarity of the NaOH solution?

c) this now standardization solution of NaOH is used to find the molecular weight of an acid H2A which has two acid hydrogen. write a balanced molecular equation for this titration reaction.

d) if 1.08 g of this acid requires 37.18 of the NaOH solution for titration to the appropriate endpoint. calculate the molecular weight of the unknown acid H2A.

A researcher was attempting to quantify the amount of DDT (dichlorodiphenyltrichloroethane) in spinach with gas chromatography using a chloroform internal standard. To begin, the researcher examined a sample containing 6.00 mg/L DDT standard and 2.50 mg/L chloroform as the internal standard, producing peak areas of 5041 and 9537, respectively. Then, the researcher collected 10.85 g of spinach, homogenized the sample, and extracted the DDT using an established method (assume 100% extraction), producing a 3.32 mL volume of unknown sample. The researcher then prepared a sample that contained 1.00 mL of the unknown sample and 1.25 mL of 10.45 mg/L chloroform, which was diluted to a final volume of 25.00 mL. The sample was analyzed using GCMS, producing peak areas of 7671 and 11805 for the unknown and chloroform, respectively. Calculate the DDT concentration in the spinach sample. Express the final answer as milligrams DDT per gram of spinach.

1. a) Predict the behavior of all five compounds (biphenyl, benzophenone, ortho-dichlorobenzene, 1-naphthol, and benzhydrol (also called "benzohydrol") on both TLC (Thin Layer Chromatography) and GC-MS (Gas Chromatography-Mass Spectroscopy). Which one do you expect to have the largest Rf on the TLC? Which one will have the smallest Rf? Which will have the longest and shortest retention times on the GC?

1. b) Ortho-dichlorobenzene has a molecular weight of 147.00 g/mol, but its MS has a very small relative abundance of the 147 peak. Instead, it has peaks at 146 (100% relative abundance), 148 (65%), and 150 (10.6%). The peak at 147 is about 6.6% as big as the 146 peak. What causes this distinctive molecular ion region for this compound? What peaks (note the plural) would you expect to see on the mass spectrum for the fragment (note the lack of plural) caused by loss of one chlorine atom (one of the C-Cl bonds breaking) during the ionization process?

1. c) For the other four compounds, note which peak on the mass spectrum you expect to corresponds to the molecular ion for the molecule, and give the approximate M+1 abundance (relative to the molecular ion) expected based on the isotopic abundance the elements present. In addition, predict at least one major fragment which you would expect for each compound.

1. d) Based on your fragmentation analysis for the previous question, describe how you would expect to be able to tell these five compounds apart by their GC-MS even if you were unable to detect the molecular ion region (that is, if all three compounds fragmented 100% of the time).

Partial Pressure/Total Pressure Question

Consider the equation:

(CH3)2N2H2(l) + 2N2O4(l) ---> 3N2(g) + 4H2O(g) + 2CO2(g)

150.0g of (CH3)2N2H2(l) reacts with excess dinitrogen tetroxide and the product gases are collected at 127°C in an evacuated 250L tank. Assuming the reaction has a 100% yield and all gases behave as ideal gas.

A) How many moles of N2 could be produced after the reaction completed?

B) What is the partial pressure of nitrogen gas produced?

C) What is the total gas pressure in the tank after the reaction?

How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 20.0 L of a solution that has a pH of 1.80?

a) What is the difference between resonance and non-resonance Raman transitions?

b) What is the difference between Rayleigh scattering, Raman-Stokes, and Raman-AntiStokes scattering?

c) Schematically plot IR spectra of a N^2, 14^NO and 15^NO. List all differences between these spectra. How many translational, rotational and vibrational degrees of freedom are in these molecules?

d) Sketch the potential that more accurately represents vibrations in diatomic molecules and compare it to the harmonic potential. Compare the energies in both cases. List all differences.

Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine (CH3CH2)3N (Kb = 5.2x10^-4), with 0.1000 M HCl solution after the following additions of titrant.

(a) 13.00 mL

(b) 20.10 mL

(c) 27.00 mL

1. Entropy (ΔS°), Enthalpy (ΔH°) and Gibb's Free Energy (ΔG°) follow Hess's law meaning their value for a reaction is the sum of the products minus the sums of the reactants. Consider the following Reaction at 25.0°C

Reaction	2Fe2O3(s)	+3C(s)	-->	4Fe(s)	+3CO2(g)
ΔH° (KJ/mol)	-824.2	0		0	-393.5
ΔS° (J/molK)	87.4	5.74		27.23	213.6

A. Calculate ΔG° where ΔG° = ΔH° - TΔS° for this reaction ___________________________

B. If 6 electrons are transferred in the balanced redox reaction above, Calculate E° for the reaction

C. Using the Nernst Equation (E = E° - (RT/nF) ln Q), what is the E value of the reaction if the partial pressure of CO₂ drops to 0.0346 atm?

D. Explain in complete sentences why this reaction is or is not spontaneous using both ΔG° , E° and E calculated above.

Consider the reaction between HCl and O2: 4HCl(g)+O2(g)→2H2O(l)+2Cl2(g) When 63.1 g of HCl are allowed to react with 17.2 g of O2, 53.8 g of Cl2 are collected. Determine the theoretical yield of Cl2 and the percent yield for the reaction.

What is the vapor pressure of an ideal solution of ethanol if 1 mile of glycerin is placed in 4 moles of ethanol at 40?C? Pure ethanol has a vapor pressure of 135.3 torr.

Calculate the pH and the pOH of an aqueous solution that is 0.035 M in HCL (aq) and 0.075 M in HBr(aq) at 25^.C.

A chemist has a substance which was either phenol or resorcinol. He puts the substance in a test tube, and puts the test tube in a beakar of boiling water. The substance melted. what was the substance and could you say whether the substance was pure or not

You are investigating the effect of strong base on the solubility of zinc hydroxide, Zn(OH)₂ (s).

(Ksp= 3 x 10^{- 15} for Zn(OH)₂ (s))

You prepare 1.0 L solution of 0.10M NaOH and add excess zinc hydroxide, Zn(OH)₂ (s).

Instead of suppresing the solubility, you observe extra solubility.

Your research advisor tells you that zinc ions react with four hydroxide ions in a solution to form the complex ion Zn(OH)₄^2- (aq).

(K_f = 2 x 10 ¹⁵ for Zn(OH)₄^2- (aq))

Calculate the pH of your solution.