The following half-reactions combine to make an electrolytic cell:

K+ (aq) + e-  K (s) E0 = −2.93

Li+ (aq) + e-  Li (s) E0 = −3.05

If a current of 1.5 Amps is placed on this cell for 5 minutes, which of the following describes the mass of solid formed (in grams) and the voltage required of the current. [1 Amp = 1 coul/s; 96500 coul = 1 mol e-]

The next 7 questions are related to the titration of 60.0 mL of a 0.0250 M Zn2+ solution with 0.0600 M EDTA in a solution buffered at pH 9. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. How many mmols of Zn2+ are present in the solution before the titration begins? What volume of the EDTA solution is needed to reach the equivalence point? What is the conditional formation constant for Zn at this pH? What is the pZn of the analyte solution before the titration begins? What is the pZn of the solution after 15 mL of titrant have been added? What is the pZn at the equivalence point of the titration? What is the pZn of the solution after 30 mL of titrant have been added?

Copper is added to steel in amounts greater than 0.2% but less than 1.5% as it strengthens, hardens and reduces corrosion of the product. The amount of copper in a steel product is determined by digesting the steel product with strong acid, converting all copper species to the Cu+1 ion, complexing the Cu+1 ion to form a light absorbing species by reaction with neocuproine, and extracting the coloured complex with isoamyl alcohol for analysis by UV/VIS spectrophotometry at the 454 nm absorbance wavelength. A 0.2108 g sample of a standard steel sample containing 0.42% of copper was analysed by the above process and a final 10.00 mL volume of the isoamyl extract was obtained. The copper complex of this solution gave an absorbance of 0.481 using a 1.00 cm cuvette. A 0.2892 g sample of a steel product that was being manufactured was analysed as above using the same procedure and equipment and a final 10.00 mL volume of the isoamyl extract was obtained. The copper complex of this solution gave an absorbance of 0.632 using a 1.00 cm cuvette. A blank solution carried through the same procedure gave an absorbance of 0.038. What is the percentage of copper in the manufactured steel product? Is the copper in this steel product within the specified range given above. Note. You have to take into consideration the absorbance of the blank solution to solve the problem.

A buffer was prepared by adding 0.1 mmoles of solid isoelectric histidine to 0.1
mmoles of solid histidine monohydrochloride and adjusting the final volume to
0.5 liters. The pKas for histidine are 1.8, 6.0, and 9.2. What is the pH of this
buffer?

At 1 atm, how much energy is required to heat 89.0 g of H2O(s) at –12.0 °C to H2O(g) at 173.0 °C?

1) All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?

2) Determine the number of protons, neutrons and electrons in (65-top) (29-bottom)X

3) What species is represented by the information: p+ = 47 n

N atoms have a high electronegativity. However, N atoms have no electron affinity, meaning that N atoms do not attract electrons. Explain how and why these facts are not inconsistent.

A solution of a theoretical triprotic acid was prepared by dissolving 4.251 g of solid in enough DI water to make 500.0 mL of solution. 13.65 mL of a 0.572 M solution was required to titrate 20.00 mL of this acid's solution.

What is the molar mass of the acid?

Consider the titration of 25.00 mL of 0.0750 M Sn²⁺ with 0.1000 M Fe³⁺ in 1 M HCl to give Fe²⁺ and Sn⁴⁺ , using a Pt electrode for the cathode and a Standard Hydrogen Electrode for the anode (connected to negative terminal of potentiometer).

e) Sketch the titration curve and indicate the equivalent pt, and the E_titr when ½ of the moles of analyte has been oxidized.

A 10.5L bulb contains NH₃ gas and HCl gas, which have equal partial pressures. The total gas pressure is 1.86atm and the temperature is 302K. These gases react completely:

            NH₃(g) + HCl(g) → NH₄Cl(s)

Calculate the mass of NH₄Cl formed.

*** Show your work

*** The answer is 21.1g but PLEASE show all of your work CLEARLY so I can understand! THANK YOU!!

3. CH3OH is synthesized via the following reaction: CO (g) + 2H2 (g)  CH3OH (g) . If the reaction occurs at 748 mmHg and 25 °C , what volume of H2 gas (in L) is necessary to synthesize 25.8 g CH3OH? What volume (L) of CO gas is required?

4. Hydrogen gas can be formed by the reaction of methane and water according to the following equation: CH4 (g) + H2O (g)  CO (g) + 3H2 (g) . In one reaction, 25.5 L of methane gas (at P = 732 Torr, T = 25 °C) is mixed with 22.8 L of water vapor (at P = 702 Torr, T = 125 °C). The reaction produces 26.2 L hydrogen gas at STP. What is the percent yield of the reaction?

Describe two chemical reactions that you encounter on a regular basis.

Figure P30.23 is a cross-sectional view of a coaxial cable. The center conductor is surrounded by a rubber layer, which is surrounded by an outer conductor, which is surrounded by another rubber layer. In a particular application, the current in the inner conductor is I₁ = 1.10 A out of the monitor, and the current in the outer conductor is I₂ = 2.84 A into the monitor. Determine the magnitude and direction of the magnetic field at point a.

A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH.

A solution is made by titrating 8.00 mmol (millimoles) of HA and 1.00 mmol of the strong base. What is the resulting pH?

More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 46.0 mL ?

No idea how to do this! Please explain..thanks!