Prove that Inter energy is Independent of the path

Determine the colligative (effective) molality of a truly saturated salt solution and the freezing point of a truly saturated salt solution (solubility limit of NaCl is 35.7 g)

Describe the trends in properties for the elements belonging to Group VI A in the periodic table. How do the following properties vary down the group?

a. Atomic Radius

b. 1st Ionization Energy

c. Electron Affinity

d. Oxidation number

e. Electronic Configuration starting from the preceding noble gas configuration

A mixture of benzene (C6H6), toluene (CH3C6H5) and methane (CH4) was injected into a gas chromatograph column that is12.5 m long. The peaks were observed at 40 s (methane), 260 s (benzene), and 272 s (toluene).

(a) Calculate the adjusted retention time (tS) and capacity factor (k) for each solute.

(b) Find the relative retention () of toluene and benzene.

(c) If the width at the base (w) of the peaks for toluene and benzene is 16 and 20 s, respectively, calculate the resolution of the two peaks.

(d) Calculate the number of theoretical plates and the theoretical plate height for toluene and benzene in this experiment.

Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. But at high temperatures, the reaction below can proceed to a measurable extent. N2(g) + O2(g) ⇔ 2 NO(g) At 3000 K, the reaction above has Keq = 0.0153. If 0.2702 mol of pure NO is injected into an evacuated 2.0-L container and heated to 3000K, what will be the equilibrium concentration of NO?

A solution contains 3.50 mol of water and 1.50 mol of nonvolatile glucose (C6H12O6).

a. What is the mole fraction of water in this solution?
b. What is the vapor pressure of the solution at 25°C, given that the vapor pressure of pure water at 25 °C is 23.8 torr?

Find the velocity of an electron emitted by a metal whose threshold frequency is 2.27×10¹⁴ s−1 when it is exposed to visible light of wavelength 5.11×10⁻⁷ m .

Please answer ALL 3 questions and provide explanations :)

4. A given mass of oxygen at room temperature occupies a volume of 500.0 mL at 1.50 atm pressure. What will be the pressure if the volume is reduced to 150.0 mL?

5. Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O₂) when stored at 22°C in a 40.0 L cylinder?

6. Consider the following reaction at STP:

CuO(s) +H₂(g) -> Cu(s) + H₂O(g)

If 40.0 g of CuO react with an excess of H₂, how many liters of H₂O will be produced?

6. A student carries out a calorimetry experiment using HCI and NaoH. What effect will each of the following have on the calculated enthalpy of the reaction relative to the actual enthalpy of reaction? (larger, smaller or no change). Explain your reasoning. a. The thermometer always registered a temperature 0.30 oc higher than the actual temperature b. The calorimeter constant used in the calculations by the student is larger than the actual value. (Hint: The best way to answer this question is to take your calorimeter constant, add at least 5 or 10 to the value and quickly redo the calculations. After completing the calculations, you should be able to complete the following statement: As the calorimeter constant increases, the calculated enthalpy of the reaction c. Unfortunately, the HCI concentration was actually 1.90 M instead of the 2.00 M HCI used in the calculations. (Hint: do a similar calculation. This is an estimate of how errors affect the result. If your data is not matching the expected values, perhaps these questions will help you understand why.)

1) A. How does the following modifications affect the rate of a square planar substitution reaction?

a) changing the trans ligand from H- to Cl-

b) changing the leaving group from Cl- to I-;

C) adding a bulky substituent to a cis ligand,

d) increasing the positive charge on the complex.

B. Organometallic compounds are heavily used in catalysis. Write out details of the reactions (including reaction cycle) in both Hydrogenation of alkanes with Wilkinson’s catalyst and Hydroformulation with cobalt carbonyl catalyst (name the catalyst in each case)

1) An unknown compound is found to burn in oxygen. When bromine is added to this unknown, the solution remains orange. What can be said about the unknown compound?

2)When a purple solution of KMnO4 is added to a different unknown, a brown precipitate forms. What can be said about this unknown?

Why is pyridine a good nucleophile for cleaving borane protecting groups from phosphanes?

3. Determine the pH (to two decimal places) of the solution that is produced by mixing 5.05 mL of 7.91×10^-5 M HI with 7.73 mL of 8.38×10^-5 M Mg(OH)₂.

Apparently a shark can smell blood up to a quarter of a mile away. How does smell travel in water? It would seem strange that if you drop ink in water it takes ages to dissipate so how can the individual particles of a smell travel so far and apparently so fast?

Explain the basis for the stacking gel portion of a polyacrylamide gel. Describe how it works with respect to the loaded protein samples as well as the running buffer components.