The data in the table below were obtained for the reaction: 2ClO2(aq) + 2OH-(aq) ---> ClO3-(aq) + ClO2-(aq) + H2O(l) Experiment number [ClO2](M) [OH-](M) Initial Rate (M/s)

1 .020 .030 .00276

2 .060 .030 .0248

3 .020 .090 .00828

a. What is the order of the reaction with respect to ClO2?

b. What is the order of the reaction with the respect to OH-?

c. What is the overall order of the reaction?

d. What is the magnitude of the rate constant for the reaction?

What is the coordination number for each of the following complexes or compounds?

1. [Co(NH3)4(H2O)2]3+[Co(NH3)4(H2O)2]3+
2. [Mg(EDTA)]2−[Mg(EDTA)]2−
3. [Cu(NH3)4]2+[Cu(NH3)4]2+
4. [Ag(NH3)2]NO3[Ag(NH3)2]NO3

Enter the coordination numbers, in the order that the complexes are listed, as four integers separated by commas (e.g., 1,2,3,4).

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Part B

What is the charge on each of the following complex ions?

1. hexaaquamanganese(II), [Mn(H2O)6]?[Mn(H2O)6]?
2. tris(carbonato)cobaltate(III), [Co(CO3)3]?[Co(CO3)3]?
3. amminepentabromoplatinate(IV), [Pt(NH3)Br5]?[Pt(NH3)Br5]?

Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).

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Part C

What is the oxidation number of the central metal ion in each of the following complexes or compounds?

1. [NiCl2Br2]2−[NiCl2Br2]2−
2. [Cr(H2O)2(NH3)4]3+[Cr(H2O)2(NH3)4]3+
3. Na[Ag(CN)2]Na[Ag(CN)2]

Express the oxidation numbers numerically, in the order that the complexes are listed, separated by commas. For a nonzero oxidation number, be sure to include the sign (e.g., +1,-2,+3).

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In glucose, which carbon is the anomeric carbon?

Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when dissolved in water.

what is the mechanism through which water activity prevents microbial proliferation?

Question 5a

1. Oxygen gas dissolves in lake water. (This is how fish get the oxygen they need to survive.) What happens to the solubility of oxygen gas when it is cold outside? Why does this happen?

   Chose from the options below. More than one answer could be correct.

   	1.	The solubility does not change.
   	2.	The solubility increases.
   	3.	The solubility decreases.
   	4.	In general, the solubility of gas solutes in liquid solvents increases as temperature decreases.
   	5.	In general, the solubility of gas solutes in liquid solvents decreases as temperature decreases.
   	6.	In general, the solubility of gas solutes in liquid solvents increases as the pressure of the gas above the liquid increases.
   	7.	In general, the solubility of gas solutes in liquid solvents increases as the pressure of the gas above the liquid decreases.
   	8.	In general, the solubility of solid solutes in liquid solvents increases as the temperature increases.
   	9.	In general, the solubility of solid solutes in liquid solvents increases as the temperature decreases.

0.8 points

Question 5b

1. Why does your pop lose it's fizz over time after the pop bottle (or can) has been opened?

   Chose from the options below. More than one answer could be correct.

   	1.	The solubility does not change.
   	2.	The solubility increases.
   	3.	The solubility decreases.
   	4.	In general, the solubility of gas solutes in liquid solvents increases as temperature decreases.
   	5.	In general, the solubility of gas solutes in liquid solvents decreases as temperature decreases.
   	6.	In general, the solubility of gas solutes in liquid solvents increases as the gas pressure above the liquid increases.
   	7.	In general, the solubility of gas solutes in liquid solvents decreases as the gas pressure above the liquid increases.
   	8.	In general, the solubility of solid solutes in liquid solvents increases as temperature increases.
   	9.	In general, the solubility of solid solutes in liquid solvents increases as temperature decreases.

PLEASE ANSWER ALL 4 THANK YOU VERY MUCH!!!!

1. How was the Periodic Table originally organized? Explain the current organization of the Periodic Table and why it is a more accurate layout of the elements.

2. What is the difference between groups and periods? What are the common names for groups IA, IIA, VIIA, VIIIA?

3. Why were elements in group 18, VIIIA, formerly known as inert gases? How is the current name of “noble gases” more appropriate? Provide examples of involved elements.

4. Hydrogen can belong to two groups on the Periodic Table, what are they? Which group do you believe hydrogen fits best in? Explain why.

A 0.100 g sample of an organic compound of an organic acid contains C, H, and O was combusted to determine the empirical formula. The combustion produced 0.2921 grams of CO2 and 0.0951 grams of H2O. Determine the number of moles of carbon in the compound, the number of moles of hydrogen in the compound, the number of grams of carbon, the number of grams of hydrogen, the number of grams oxygen as well as the empirical formula. The molecular weight of the compound was found to be 660 grams per mole, determine the molecular formula.

A gas with 65% hydrogen exits a reactor at 2310 psia and 700°F. Select an appropriate material for the piping at the exit of the reactor. (Hint: Find a good version of the Nielson Curves).

While OLEDS are useful, sometimes they can be hard to convert to regular devices.

1)Are OLED's more or less robust than inorganic LEDS and why?

2) If a defect, for example a disruption in the conjugation of a polymer occurred, how would this change the light emitting properties of the material?

3) If lemon juice was spilled on your phone (aq citric acid) Draw the repeating unit of PPV and the mechanism of this species with aqueous acid. Would a defect occur? How likely is the reaction and name a common species in everyday life that can react with systems such as these.

If a solution containing 17.91 g17.91 g of mercury(II) perchlorate is allowed to react completely with a solution containing 5.102 g5.102 g of sodium dichromate, how many grams of solid precipitate will be formed?

mass:

gg

How many grams of the reactant in excess will remain after the reaction?

mass:

gg

Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles.

Hg2+Hg2+:

molmol

ClO–4ClO4–:

molmol

Na+Na+:

molmol

Cr2O2−7Cr2O72−:

mol

Explain the strengthening mechanism in the large particle and dispersion strengthen composites with their differences.

One can argue that both nitric oxide and sulfur dioxide are natural, and hence, harmless. Would you agree or disagree with this statement? Explain using the concept of equilibrium and biogeochemical cycles, and discuss their effects on natural waters.

Describe how you would design the experiment, what you would measure, and how you could determine the specific heat capacity of water.