1. An electrochemical cell is based on the following two half-reactions:
Ox: Pb(s)→Pb2+(aq, 0.18 M )+2e−
Red: MnO−4(aq, 1.50 M )+4H+(aq, 1.8 M )+3e−→
MnO2(s)+2H2O(l) Compute the cell potential at 25 ∘C.

2.A concentration cell consists of two Sn/Sn2+ half-cells. The cell has a potential of 0.16 V at 25 ∘C.

What is the ratio of the Sn2+ concentrations in the two half-cells?

Express your answer using two significant figures.

3.Metal plating is done by passing current through a metal solution. For example, an item can become gold plated by attaching the item to a power source and submerging it into a Au3+ solution. The item itself serves as the cathode, at which the Au3+ions are reduced to Au(s). A piece of solid gold is used as the anode and is also connected to the power source, thus completing the circuit.

What mass of gold is produced when 8.80 A of current are passed through a gold solution for 18.0 min ?

Express your answer with the appropriate units.

A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted to lead(II). This reaction is facilitated by the presence of sulfuric acid, H2SO4, as shown by the reaction

Pb+PbO2+2H2SO4→2PbSO4+2H2O

Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 3.60 A of current is drawn from the battery for 6.00 hours ?

Consider the titration of 25.0 mL of 0.175 M cyanic acid, HCNO, with 0.250 M LiOH. The Ka of HCNO is 3.5 * 10^-4.

What is the volume of LIOH required to reach the equivalence point?
b. calculate the pH after the following volumes of LIOH have been added:
a. 0mL
b. 5.0 mL
c. 8.75 mL
d. 17.5 mL

10. How much methanol (CH₃OH, in grams) can be formed from 49.2 mg of hydrogen? Assume excess CO.

CO(g) + 2H₂(g) → CH₃OH(g)

-Consider the following balanced chemical equation: 2N₂H₄(g) + N₂O₄(g) → 3N₂(g) + 4H₂O(g)

a. How many moles of water form from 0.438 moles of N₂O₄?

b. How many moles of water form from 0.438 moles of N₂H₄?

c. How many moles of nitrogen form from 0.438 moles of N₂O₄?

d. How many moles of nitrogen form from 0.438 moles of N₂H₄?

What is the enthalpy of the following reactions? Use the appendix in your text book using heat formatino values.

1. SO3+ H2O-----H2SO4

2. 3K2O2+3H2O----6KOH+O3

3. Fe3O4+8HCL----2FeCl3+FeCl2+4H2O

1: Select all of factors that affect the rate of a chemical reaction:

Why is the region of the electromagnetic spectrum between 8 and 13 um known as the "atmospheric window"? Why are gases that absorb thermal IR in this range of particular concern? What are some of those gases?

A.) Write the equation which describes the reaction between crystal violet and hydroxide ion.

B.) A solution is prepared by mixing 25.0 mLs of 4.84*10^-6 M crystal violet solution with 20.0 mLs of 0.10 M NaOH solution and diluted to a final volume of 100.0 mLs. Determine the limiting reagent.

C.) After the reaction has gone to completion, calculate the concentration of all species in the reaction.

D.) How does the concentration of sodium hydroxide change over the course of the reaction?

E.) Explain your answer in question D in terms of the intial concentrations of reactants.

2,2,4-trimethylpentane

A) one retrosynthetic analysis

B) a reaction scheme showing each of the synthetic steps with starting materials, products, reagents and conditions

C) a paragraph or so describing the logic of a synthetic strategy and why it would be the most likely to give

the desired product.

D) References to any sources that were used.

In a constant-pressure calorimeter, 75.0 mL of 0.830 M H2SO4 was added to 75.0 mL of 0.400 M NaOH. The reaction caused the temperature of the solution to rise from 21.85 °C to 24.57 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·K, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

Acid base titration determination of Na2CO3 in Soda Ash

CO3^2- +H⁺ = HCO3^-

HCO3^- + H⁺ = H2CO3

Buffer by mixing acetic acid and sodium acetate.

The comparison indicator solution should match the analytical solution at the second equivalence point in three respects: pH, Ionic strength, color and intensity

A) Calculate the concentration of sodium acetate necessary to achieve the ionic strength in pre lab 4. ( Pre lab 4 calulation, the ionic strength that I have calculated is to be 0.1)

B) Calculate the concentration of acetic acid given the values calculated for A.

C) Calculate the mass of unknown to weight out in order to consume 40 ml of 0.1 M HCL assuming the unknow is 35% by mass Na2CO3.

For preview calculation where you calculate the mass of Na2CO3 needed to consume 40 mL of 0.10 M HCL in a titration of Na2CO3 with HCL come out to be 0.212 gram needed to consume 40 mL of 0.10 M of HCL.

"monoclonal antibody can be used as a therapeutic agent for the treatment of cancer"- justify the statement with an appropriate example

If the weight of an unknwon sample is greater than 1g, as it may be with pottassium phthalate samples of low percentage purity, why does this sample need only to be weighed to the nearest milligram?

Evaluate the physical and chemical methods of waste treatment? How efficient are they in and what is their effect on the environment (positive and/or negative)?

B.) Enter the net ionic equation representing aqueous acetic acid neutralized by aqueous barium hydroxide.   

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.\

C.) Enter the molecular equation representing solid chromium (III) hydroxide reacting with nitrous acid.   

Express your answer as a balanced molecular equation. Identify all of the phases in your answer.

D.) Enter the net ionic equation representing solid chromium (III) hydroxide reacting with nitrous acid.   

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.

E.) Enter the molecular equation representing aqueous nitric acid and aqueous ammonia reacting.

Express your answer as a balanced molecular equation. Identify all of the phases in your answer.

F.) Enter the net ionic equation representing aqueous nitric acid and aqueous ammonia reacting.  

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.