Calculate the values of Delta G and Ecell for the following reaction, label the half reactions as anode and cathode.

2Ag(s) + Cu²⁺ (aq) > 2 Ag⁺ (aq) + Cu(s)

* My main question lies in which is cathode and anode...it seems that the Ag half reaction (2Ag(s) > 2Ag⁺ +2e-) signifies Ag(s) loosing electrons causing the positive reactant, this leads me to think loss of electrons/this is the oxidation half reaction, therefore Ag(s) is the reduction agent and anode with a given appendix value of 0.800V, BUT when I look at my professors notes he signifies that the Cu²⁺(aq) half reaction (Cu²⁺  + 2e- > Cu(s)) is the anode with a appendix value of 0.342V.

To me the Cu²⁺ gains electrons and is the reduction reaction/cathode - why am I wrong, is it because the Ag value is the more positive of the two? and if this is so... When am I to determine the cathode/anode label with the "more positive" logic?

WORD BANK

a. Aqueous Solutions

b. Colligative Properties

c. Concentrated Solution

d. Dilute Solution

e. Electrolytic Solution

f. Hydration

g. Immiscible

h. Insoluble

i. Miscible

j. Molality (m)

k. Molarity (M)

l. Non-electrolyte Solution

m. Osmotic Pressure

n. Osmosis

o. Percent by mass

p. Percent by volume

q. Recrystallization

r. Salvation

s. Saturated

t. Semipermeable Membrane

u. Solubility

v. Soluble

w. Solute

x. Solution

y. Solvent

z. Supersaturated Solution

aa. Unsaturated

Use the Vocabulary words above to complete the following sentences words can be used more than once, some words are not be used.

A ___________ is an intimate homogeneous mixture of a solute and a solvent.

The substance being dissolved in a solution is the __________.

The substance whose physical state is retained is the __________.

If a solute will dissolve in a given solvent it is said to be ________ in that solvent.

If the solute does not dissolve in the solvent the solute is _________.

The __________ of a substance is a measure of how much solute will dissolve in a given quantity of solvent at a specific temperature.

When two liquids dissolve in each other they are __________; if they do not, then they are ________.

A ___________ __________ is one that has a relatively large amount of solute dissolved in it.

A ___________ ___________ has a relatively small amount of solute dissolved in it.

The process by which water molecules surround the ions of the solute is called __________, for any other solvent except water the term is ________.

A solution at a given temperature that exists in dynamic equilibrium with undissolved solute is said to be ___________.

When a solution contains less solute than the solubility limit, it is said to be _____________.

A ____________ _______ contains more than the maximum amount of solute for a given temperature.

A solution containing a solute that dissociates into ions is called an __________ ___________.

A solute that dissolves into nonconductive particles is called a____________ ____________.

A common way to purify a mixture of two solids that have different solubilities is called __________.  

#3-c Post-lab exp. 24

3. Concerning the applicability of the titration method, comment on if and how you could use it to determine K_sp for the following:

c. copper (II) iodate

An ideal gas (which is is a hypothetical gas that conforms to the laws governing gas behavior) confined to a container with a massless piston at the top. (Figure 2)  A massless wire is attached to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.90 to 2.45L . When the external pressure is increased to 2.50 atm, the gas further compresses from 2.45 to 1.96L .

In a separate experiment with the same initial conditions, a pressure of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.90 to 1.96L in one step.

If the final temperature was the same for both processes, what is the difference between q for the two-step process and q for the one-step process in joules?

Express your answer with the appropriate units.

Two chemicals A and B are combined to form a chemical C. The rate, or velocity, of the reaction is proportional to the product of the instantaneous amounts of A and B not converted to chemical C. Initially, there are 100 grams of A and 50 grams of B, and for each gram of B, 2 grams of A is used. It is observed that 25 grams of C is formed in 10 minutes. How much is formed in 40 minutes? (Round your answer to one decimal place.)


What is the limiting amount of C after a long time?


How much of chemicals A and B remains after a long time?

t =  min
At what time is chemical C half-formed?

A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ?C . The initial concentrations of Ni2+ and Zn2+ are 1.80M and 0.110M , respectively. The volume of half-cells is the same.

A.What is the initial cell potential?        

B. What is the cell potential when the concentration of Ni2+ has fallen to 0.600M ?        

C. What is the cell potential when the concentration of Ni2+ has fallen to 0.600M ?        

D. What is the concentration of Zn2+ when the cell potential falls to 0.45V ?

Thank you.

Nucleophilic Substitution Reactions Organic Chemistry Lab:

Explain the order of elution you observed while performing the gas chromatography for this experiment. What property of the product molecules seem to be the most important in determining relative retention times?

What is the functions of the following:

bicarbonate ion

calcium ion

chloride ion

magnesium ion

phosphate ion

potassium ion

sodium ion

sulfate ion

Thank you

Calculate the Molar Mass for the following compounds:

Fe3 (PO4)2

(NH4)2S

Zn (C2H3O2)2

Assume you have a mixture of benzophenone, diphenylmethanol and biphenyl that you have placed (spotted) on a TLC reverse phase gel (non-polar stationary phase) plate. If you developed the plate in methanol (mobile phase) which compound would have the highest R_f value? Explain your reasoning to support your answer.

1) Provide brief definitions for the following: a) conjugation; b) polymer, c) HOMO and LUMO.

2) Why do conjugated compounds absorb light in the Ultraviolet region? Why do more conjugated compounds absorb at higher wavelengths/lower energies? What is required for organic compounds to absorb in the Visible light region?

Consider a 300mL sample of 0.250M HCN (Ka=4.9x10^-10). To find the pH, do you need an ice table, can you use the Henderson-Hasselbalch equation, or something else? If an ice table, will it be a Ka or Kb equilibrium? Can you use the small x assumption? Is this a buffer? If something else, then how?

(Need Help Please!!! If possible could you work it out so i can know how to do it)

A certain weak base has a Kb of 8.00

Two 20.0-g ice cubes at –13.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

Heat capacity of H2O(S) is 37.7 J/(mol X K); Heat Capacity of H2O(l) is 75.3 J/(mol X K); Emthalpy of Fusion of H2O is 6.01 kJ/mol

This is for a titration experiment starting with 25 ml of HCL. I've answered two but am struggling with the others.

2. Find the equivalence point on the graph. What is the equivalence volume of NaOH at this point?

The pH at the equivalence point is 8.77 and the volume of NaOH at this point is 40.00 mL of NaOH

3. a. Calculate the unknown molarity of the diluted acetic acid from the volumes of acid and base at the equivalence point and the molarity of the NaOH M_a × V_a = M_b × V_b.

b. Once you find the molarity of your diluted solution use that to calculate the molarity of the original solution using the equation M₁ × V₁ = M₂ × V₂ a second time.

4. In experiment 1, you were able to calculate the concentration of the HCl solution using the initial pH. Would this same approach work with the acetic acid? Why or why not?