A little stuck, could you please show working out?

Which of the following processes represents an oxidation reaction?

Which one of the following processes represents a reduction reaction?

50lbs of gas with the specific gavity of .88(treat as real gas) is in a tank at p=1384 psig and at T=320F what is volume of the tank in ft^3        This question is in oilfield units

Using a table of standard electrode potentials, decide which of the following statements is completely true.

A. Cu2+ can oxidize H2, and Fe can reduce Mn2+ .

B. Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+ .

C. Fe2+ can oxidize H2, and Fe2+ can reduce Au3+ .

D. Br2 can oxidize Ni, and H2 can reduce Mn2+ .

E. H + can oxidize Fe, and Ni can reduce Br2.

Answer: E.. but why? can you explain why A-D are incorrect and why E is right. I know it has something to do with how they are positioned on the standard reduction potential list, but I dont understand the concept, which I will need to know for my exam. thank you!

Under the topic of aqueous chemical equilibria, outline the quantitative treatment of a single acid in solution. Indicate in your answer, where a mass balance expression is utilised.

Please write (For each) the resulting reactions, molecular equations, ionic equatons, and net ionic equations. No need to show work. Thank you!

[1] copper(II) sulfate + sodium hydroxide

[2] copper(II) sulfate + sodium carbonate
[3] copper(II) sulfate + lead(II) nitrate
[4] copper(II) sulfate + barium chloride
[5] copper(II) sulfate + sodium phosphate
[6] sodium carbonate + sulfuric acid
[7] sodium carbonate + hydrochloric acid
[8] cadmium(II) chloride + sodium sulfide
[9] cadmium(II) chloride + sodium hydroxide
[10] nickel(II) chloride + sodium acetate
[11] nickel(II) chloride + silver(I) nitrate
[12] nickel(II) chloride + sodium carbonate
[13] sulfuric acid + sodium hydroxide
[14] sulfuric acid + sodium acetate
[15] ammonium chloride + sodium hydroxide
[16] barium chloride + sodium phosphate
[17] lead(II) nitrate + sulfuric acid
[18] lead(II) nitrate + sodium sulfide
[19] sodium sulfide + hydrochloric acid
[20] potassium chloride + sodium nitrate

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g of NH3. If the total pressure of the mixture is 3.05 atm, what is the partial pressure of each component?

At 650 K, the reaction MgCO3(s)?MgO(s)+CO2(g) has Kp=0.026. A 12.8L container at 650 K has 1.0g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.900L .

Find the mass of MgCO3 that is formed.

Consider the titration of a 27.3 −mL sample of 0.125 M RbOH with 0.105 M HCl. Determine each of the following.

1. the initial pH

2. the volume of added acid required to reach the equivalence point

3.the pH at 5.6 mL of added acid

4. the pH at the equivalence point

5. the pH after adding 4.9 mL of acid beyond the equivalence point

You add 0.535 g of NaOH to 100.0 mL of water at 25

An organic compound contains carbon, hydrogen, and sulfur. A sample of it with a mass of 2.712 g was burned in oxygen to give gaseous CO₂, H₂O, and SO₂. These gases were passed through 311.2 mL of an acidified 0.0200 M KMnO₄ solution, which caused the SO₂ to be oxidized to SO₄^2-. Only part of the available KMnO₄ was reduced to Mn²⁺. Next, 31.12 mL of 0.0300 M SnCl₂ was added to 31.12 mL portion of this solution, which still contained unreduced KMnO₄. There was more than enough added SnCl₂ to cause all of the remaining MnO₄^- in the 31.12 mL portion to be reduced to Mn²⁺. The excess Sn²⁺ that still remained after the reaction was then titrated with 0.0100 M KMnO₄, requiring 0.02095 L of the KMnO₄ solution to reach the end point. Based upon all this data, the percentage of sulfur in the original sample of the organic compound that had been burned is___%.

The iodination of acetone, CH3COCH3, in aqueous solution is catalyzed by the hydrogen ion H+:

I2+CH3COCH3H+?HI+CH3COCH2I

The reaction can be followed visually by adding starch. The purple starch-iodine complex forms immediately, then disappears when the iodine has been consumed. The kinetics of the reaction may be determined by recording the time required for the color to disappear, which is the time required for the iodine, I2, to be consumed.

The following data were acquired in an iodination experiment involving acetone. All reaction times are in terms of the rate of disappearance of I2.

part A

In the general rate law

rate=k[I2]^X[H+]^Y[CH3COCH3]^Z

what are the values of X, Y, and Z?

how to calculate the equilibrium concentration using absorption data and the best fit line from the beer's law

5. If the sulfuric acid and nitric acid in rainwater are capable of adversely affecting soil, trees, and fish, why doesn’t this same acid adversely affect people when they walk in the rain? 6. Which do you feel is likely to be more acidic: acid rain or acid fog? Explain your reasoning.

EXPERIMENT #4 – PREPARATION OF o-CHLOROBENZOIC ACID

1. PREPARE A SOLUTION OF CuCl AS FOLLOWS: Dissolve CuSO4∙5H2O (2.34 g) and pure NaCl (0.62 g) in water (8 mL) in a 50 mL Erlenmeyer flask. Warm on a hot plate to dissolve. Add a solution of sodium bisulphite (0.56 g) in water (6 mL) to the hot solution, with constant shaking over a period of about 5 minutes. Cool to room temperature in an ice bath, and decant the supernatant liquid from the colourless CuCl. Wash the precipitate twice by decantation with water containing a little (approximately 1% (v/v) solution) sulphurous acid (HSO3 ‐ + H+ →H2SO3), to prevent oxidation. Dissolve the CuCl in concentrated HCl (4 mL). Stopper the flask and cool in an ice‐salt mixture (0‐5oC) while the diazonium salt is being prepared.

2. PREPARE A DIAZONIUM SALT AS FOLLOWS: In a 125 mL conical flask, dissolve o‐ aminobenzoic acid (anthranilic acid, 0.94 g) in a solution containing conc. HCl (1.4 mL) and water (8.2 mL). Cool the solution to 0 oC. Slowly add a cold solution of NaNO2 (0.46 g) in water (1.6 mL). Do not allow the temperature to rise above 10 oC during this procedure. Add a small amount of urea (a few crystals) to the mixture and cool the resulting solution in an ice bath.

3. PREPARE o-CHLOROBENZOIC ACID AS FOLLOWS: Transfer the cold CuCl solution to a 150 mL beaker. Slowly add, with stirring (use long glass rod), the cold diazonium salt solution to the cold CuCl solution. Watch for foaming. Allow the mixture to stand for 20 minutes at room temperature with frequent stirring. Vacuum filter the precipitated o-chlorobenzoic acid and wash the product with a small amount of cold water.

4. RECRYSTALLIZE AS FOLLOWS: Clean the Buchner funnel and place it along with a 500 mL vacuum flask into the oven at 105 oC. In a 150 mL beaker, add the crude product, a small amount of charcoal, water (~20 mL) and ethanol (~2.6 mL). Heat to a gentle boil, stirring the mixture periodically. When the product has dissolved, quickly filter through the hot Buchner funnel (PRERINSE FILTER PAPER WITH BOILING WATER) in order to remove the charcoal before the o‐chlorobenzoic acid is allowed to 26 crystallize. Allow to cool to room temperature. Vacuum filter the recrystallized product. Dissolve a few crystals of the product in ethanol and spot it on a TLC plate and label it “R”. Likewise dissolve a few crystals of anthranilic acid in ethanol and spot that on a TLC plate as well, labelling it as “SM”. Develop the TLC plate as usual, taking note of the solvent used. Determine the m.p. and percent yield of the dried product next week while doing experiment #5.

If the experiment were to be performed exactly this way, how would one determine the limiting reagent of the reaction for the percent yield calculation? What should be the limiting reagent of this reaction? When I ran this experiment, I was able to form 0.43 g of product.

Thanks for your help!