Use both the van der Waals and the Redlich-Kwong equations to calculate the molar volume of CO at 200K and 1000bar. Compare your result to the result you would get using the ideal gas equation. The experimental value is 0.04009 L-mol-1

Please explain each step.

for each of the following electromagnetic radiation sources, tabulate the frequency (Hz), the wavenumber, the energy (eV), and the region of the electromagnetic spectrum (IR, vis, etc.)

a. frequency doubled Nd:YAG laser at 532nm

b. CO2 laser at 10.6 micrometers

c. klystron at 1.23 cm

d. Cu K(alpha) emission at 154.1 pm

e. oscillator used in NMR at 1.5m

1- Brief discussion of column chromatographic separation (solvent polarity, elution of compounds etc.)

2- Relationship between polarity and thin layer chromatography​.

1- Brief discussion of column chromatographic separation (solvent polarity, elution of compounds etc.)

2- Relationship between polarity and thin layer chromatography​.

Part B

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH.

Express your answer numerically

Part C

A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 21.0 mL of HNO3.

Express your answer numerically.

Part D

A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 25.0 mL of NaOH.

Express your answer numerically.

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MW (g/mol) / MP ( oC) / Solubility in cold H2O (g / 100 mL) / Solubility in boiling H2O (g / 100 mL)

Acetanilide 135.2 / 114 / 0.54 / 5.0

Phenacetin 179.2 / 135 / 0.076 / 1.22

Using solubility data in the table of reagents, calculate the minimum amount water needed to recrystallize:

i. 1.5 g of phenacetin.

ii. 1.5 g of acetanilide.

b. If the minimum amount of water needed is used, how many grams of each compound would crystallize out of solution following the recrystallization?

i. phenacetin

ii. acetanilide

At what pressure does the boiling point of water become 350°C? If oceanic pressure increases by 0.5 atm for every 5 m, to what ocean depth does this pressure correspond? ΔHvap,m for water is 44.03 kJ/mol.

Ammonia gas will react with oxygen gas to yield nitrogen monoxide gas and water vapor. write balanced chemical equation, how many moles of ammonia will react with 6.73g oxygen?

the heat of fusion of ice is 6.00 kj/mol. what number of photons of wavelength = 6.42×10e-6m are needed to melt one gram of ice?

A piece of magnesium can be attached to the iron hull of a boat to prevent it from rusting.

Why is the magnesium called a sacrificial metal?

How does the Mg keep the iron hull from rusting?

Which can be thought of as the positive cathode, the Mg or the steel hull? Explain.

Putting a block of Mg on a steel boat hull does not create a battery. Why not?

A mixture of 0.2063 mol of Cl2, 0.2093 mol of H2O, 0.1887 mol of HCl, and 0.09871 mol of O2 is placed in a 1.0-L steel pressure vessel at 575 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.05821 mol of O2 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. (b) Calculate KP for this reaction.

What is the differnce between linear synthesis and convergent synthesis? Why is convergent synthesis in general favored over linear synthesis and When would linear synthesis be used?

7. A piece of zinc metal with a mass of 35.0 g is heated in boiling water to 101.3 ºC and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 23.8 ºC. When thermal equilibrium is reached, the final temperature is 27.0 ºC. Calculate the specific heat capacity of the zinc.

Consider the following reaction between oxides of nitrogen:NO 2 1 g 2 + N 2 O 1 g 2 ¡ 3 NO 1 g 2 (a) Use data in Appendix C to predict how ∆ G for the reac-tion varies with increasing temperature. (b) Calculate ∆ G at 800 K, assuming that H ° and S ° do not change with tem-perature. Under standard conditions is the reaction sponta-neous at 800 K? (c) Calculate ∆ G at 1000 K. Is the reaction spontaneous under standard conditions at this temperature?