Would a molecular orbital diagram be appropriate to describe bonding in Ti? Explain.

I know what an Electrolyte and a non-electrolyte is, but how do I relate the number of particles in a given solution to the type of solute (electrolyte or non-electrolyte).

What is an element that shares group properties with Mg? What properties are common in this group?

What is a buffering region?

What is the Bohr Effect?

1. Describe the scope (types of R groups etc.) advantages and limitations (functional group tolerance, solvent considerations, air/water sensitive etc.) for the Heck coupling reaction.

2. What is the relative reactivity of aryl halogens in Heck coupling and what specific step in the mechanism is affected?

Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2→2SO3.

Part A How many O2 molecules are needed to react with 5.69 g of S? Express your answer numerically in units of molecules.

Part B What is the theoretical yield of SO3 produced by the quantities described in Part A? Express your answer numerically in grams.

Limiting reactant

Next, consider a situation in which all of the S is consumed before all of the O2 reacts, or one in which you have excess S because all of the O2 has been used up.

Part C For each of the given situations, indicate whether S or O2 is the limiting reactant.

Drag each item to the appropriate bin.

3.0 mol sulfur 3.0 mol oxygen 3.0 mol sulfur 4.0 mol oxygen 3.0 mol sulfur 5.0 mol oxygen

Bin 1: Limiting reactant is sulfur

Bin 2: Limiting reactant is oxygen

1. please explain the reason behind ruthenium ligand rate. a) why is it slow? b) what does geometry has to do with the slow rate c)what is the role with thermodynamics and kinetics?

2)what effect will this have on cancer treatment?

3) what is preferred for cancer treatment slow or fast ligand exchange and why?

1. Give examples of three important types of chemical reactions that occur in biochemical systems.

2. How is a standard thermodynamic state defined for biochemical systems?

3. Explain what is meant by a term "substrate cycle."

4. What is the critical limitation for formation of carbon-carbon bonds in biochemical systems?

5. Explain why most fatty acids within the body have an even number of carbon atoms.

6. List three vital functions served by amino acids in the body.

3. Use the information in problem 1 and the experimental data from a tracer study shown in the table below to answer the following questions.

a).   (2 pts) To determine the required free chlorine for disinfection of the filtered water, a tracer (fluoride ion, dosage = 6.0 mg/L) study (step-dose method) was used to determine t₁₀. What is the t₁₀?

b). (15 pts) During the year the water temperature mostly ranges from 5 to 20^oC. Assume the pH value of water is relatively stable at about 8.0 at 5^oC and about 7.5 at 20^oC during the disinfection process. What is the maximum difference (mg/L) of required free chlorine due to the range of water temperature?

c).   (9 pts) The minimum required chlorine residual in the plant effluent is 0.2 mg/L. Does the minimum free chlorine calculated in part b satisfy the requirement? Assume the distribution pipeline is an ideal PFR and free chlorine decays following a first-order reaction with a reaction rate constant k (0.12 hr^-1 at 5^oC and 0.15 hr^-1 at 20^oC) and the average velocity of treated water along the pipe is about 3 ft/s. If a chlorine residual above 0.6 mg/L is too objectionable to be accepted, what will be the minimum pipe distance from the plant to the nearest consumers required to address the odor/taste issue in cold weather? What will be the maximum service distance to ensure minimum chlorine residual 0.1 mg/L in destination in warm weather?

d).        (6 pts) The plant (based on the above conditions) will provide service to some consumers only 2 mile (of pipeline) away. The treatment plant will build an additional tank at the end of the pipeline to temporally store treated water between the consumers and the plant. Assume the tank is an ideal CMR and the decay rate is 0.12 hr^-1 based on a first-order reaction (independent from the temperature) and the pipeline remains as 2 mile. What should be the minimum hydraulic residence time of this tank?

[8] What are acids and bases? Describe the two terms giving examples that you commonly use. Explain the term ‘pH’, its equation, and provide a few numbers representing the pH scale! Explain the term ‘Acid Rain’, its formation and its detrimental effect on environment.

Phosphoric acid is a triprotic acid (Ka1=6.9×10−3Ka1=6.9×10−3, Ka2=6.2×10−8Ka2=6.2×10−8, and Ka3=4.8×10−13Ka3=4.8×10−13).

To find the pH of a buffer composed of H2PO−4(aq)H2PO4−(aq) and HPO2−4(aq)HPO42−(aq), which pKaKa value should be used in theHenderson–Hasselbalch equation?

pKa1Ka1 = 2.16

pKa2Ka2 = 7.21

pKa3Ka3 = 12.32

Calculate the pH of a buffer solution obtained by dissolving 18.018.0 g of KH2PO4(s)KH2PO4(s) and 30.030.0 g of Na2HPO4(s)Na2HPO4(s) in water and then diluting to 1.00 L.

pH=

Potassium nitrate, KNO3KNO3, has a molar mass of 101.1101.1 g/mol. In a constant-pressure calorimeter, 44.644.6 g of KNO3KNO3 is dissolved in 201201 g of water at 23.00 °C23.00 °C.

KNO3(s)H2O−−→K+(aq)+NO−3(aq)KNO3(s)→H2OK+(aq)+NO3−(aq)

The temperature of the resulting solution decreases to 17.70 °C17.70 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g⋅°C)4.184 J/(g·°C), and that there is negligible heat loss to the surroundings.

How much heat was released by the solution?

What is the enthalpy of the reaction?

In isolated thylakoid membranes you measure, through the use of molecular probes, a transmembrane potential of delta psi = + 60 mV and a delta pH of 2- (inside acidic) across the thylakoid membrane. A) How much free energy is yielded by moving 1 mole of protons outward through the H+-ATPase under these conditions of delta psi and delta pH? B) If there are 10 c- subunits in the chloroplast ATPase (cFo), how much energy is available to synthesize each ATP?