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.

29. How propyl amine can be synthesized by Gabriel Synthesis? Write the mechanism of the reaction.

30. How reductive amination methodology can be applied for the synthesis of the potent CNS drug “Amphetamine”?

31. Write note on “Sandmeyer reaction”. Write down the mechanism of formation of p-Bromotoluene from pMethylaniline.

Al₂(CO₃)₃ (s) è Al₂O₃ (s) + 3 CO₂ (g)           ∆H = +579 kJ            

a. What kind of chemical reaction is taking place? Is it endo- or exothermic? Explain how you know both answers.

b. Predict the change in enthalpy for each of the following reactions:

          1. 5 Al₂(CO₃)₃ (s) è 5 Al₂O₃ (s) + 15 CO₂ (g)           ∆H = ??

          2. 3 Al₂O₃ (s) + 9 CO₂ (g) è 3 Al₂(CO₃)₃ (s)             ∆H = ??

          3. Write the balanced thermochemical equation that will have ∆H = -2316 kJ

c. How much heat is required to react 5.00 grams of the aluminum carbonate?

d. If 5250 kJ of heat is added to aluminum carbonate, how many grams of aluminum oxide will be produced?

e. Using the enthalpies of formation found in the appendix of your textbook and the thermochemical equation above, calculate the enthalpy of formation of solid aluminum carbonate

Propane gas is used as a propellant in aerosol cans.

a. Suppose a 455 mL container contains propane gas at a pressure of 1.75 atm at 25.0 ^oC. How many grams of propane are in the container?

b. If the can in part a is cooled to 5.0 ^oC and an additional 10.0 grams of propane is added to the can, what is the pressure of the propane gas? How does this pressure compare to the original pressure in part a? Whose law(s) explains this change and use the postulates of Kinetic Molecular Theory to explain the change.

c. If all the propane in the original can (as described in part a) were transferred to a balloon at STP, what volume would the propane occupy? How does this compare the original conditions in part a? Explain in terms of Kinetic Molecular Theory and gas laws.

d. The can in part a says that it can handle a pressure of 5.00 atm without bursting. What is the maximum mass of propane the can is able to hold before bursting? Whose law describes the relationship and explain the change using Kinetic Molecular Theory.

e. The can in part a says that it can handle a pressure of 5.00 atm. What is the maximum temperature to which the propane can be heated to without bursting.

a) The complete combustion of 10.0 g of solid naphthalene requires what volume of oxygen gas at 20.0 ^oC and 1.00 atm? How much heat energy will be transferred in this trial? Specify direction of heat transfer in your answer.

b) If the water vapor and carbon dioxide gas produced in the trial described in part d. is collected in a 20.0 L container at 427 ^oC and this container can only withstand a maximum of 5.00 atm of pressure, will the container stay intact or explode

C₁₀H₈ (s) + O₂ (g)   è CO₂ (g) + H₂O (g)    

In terms of entropy and the real world, what is the end result of a spontaneous process?

Part A

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 18.0 mL of KOH.

Part B

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 13.0 mL of HNO3.

Part A

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.