1. Electrolytic reactions, like other chemical reactions, are not 100% efficient. In a copper purification apparatus depositing Cu from a CuSO4 solution, operation for 5.47 hours at a constant current of 5.45 A deposits 29.2 g of Cu metal. What is the efficiency?

b) How long would it take to electroplate all the Zn²⁺ in 0.280 L of 0.210 M ZnSO₄ solution with a current of 2.35 A?

please answer both A and B

1. Please explain why “noncompetitive inhibition”- where it is observed experimentally- is more likely to be a coincidence than a reveal of something profound in the mechanism of an enzyme (in contrast to competitive and uncompetitive inhibition).

Please show all work!

Balance the following reaction in a basic solution:

Ag(s)+Zn^2+(aq)--->Ag2O(aq)+Zn(s)

Use the following half-reactions to write three spontaneous reactions, and calculate E cell for each reaction:

a. Au⁺ (aq) + e^- ----> Au (s) E= 1.69 V

b. N₂O (g) + 2H⁺ (aq) + 2 e^- ----> N₂ (g) + H2O (l) E= 1.77 V

c. Cr³⁺ (aq) + 3e^- ---> Cr (s) E= -0.74 V

What do you understand by " hydrated ions" ? Give examples of hydrated ions and explain at least one hydrated ion's sturcture and formation.

1.) For the chemical reaction 2 Al + 3 H 2 SO 4 ⟶ 3 H 2 + Al 2 ( SO 4 ) 3 what mass of hydrogen is produced from 1.97 mol of aluminum?

2.) Convert 1.77×1024 atoms of carbon to moles of carbon.

1.77×1024 atoms=

3.)

Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline.

2C8H18+25O2⟶16CO2+18H2O

How many moles of CO2 are emitted into the atmosphere when 17.1 g C8H18 is burned?

4.) For the reaction

2KI+Pb(NO3)2⟶PbI2+2KNO3how many grams of lead(II) iodide, PbI₂, are produced from 89.7 g of potassium iodide, KI?

5.)For the reaction

2NaOH+H2SO4⟶Na2SO4+2H2O

how many grams of sulfuric acid, H₂SO₄, are needed to react completely with 33.1 g of sodium hydroxide, NaOH?

PLEASE HELP...

Calculate the value of deltaG for the reaction

Si3N4 + 3O2 = 3 SiO2(alpha-quartz) + 2 N2

at 800 K. What percentage error occurs if it is assumed that deltaCp for the

reaction is zero?

The vapor pressure of chloroform (CHCl3) is 173 mm Hg at 25 °C. What is the vapor pressure of a solution consisting of 268 g of chloroform and 0.129 mol of a nonvolatile nonelectrolyte?

At the extreme limits (high and low end) of the plot of pH vs. log([HPO42-]/[H2PO4-]), the data points may appear as though they are leveling off. Think about the [HPO42-]/[H2PO4-] ratio at the extreme limits and explain why this leveling off occurs. (There is one other answer on Chegg but I do not understand the logic of that response) Thank you!

Research Question: How to determine the quantity of polyphenol oxidase in apple juice?

Over the course of the semester, we studied several techniques (spectrophotometry, acid-base titrations, redox experiments) to answer questions related to quantification and identification of compounds, kinetics of chemical reactions,and equilibrium constants. With some background research, write a researchable question that could be answered with one or more of the techniques used during the semester.Write a research plan to answer the question. The plan does not have to be a detailed step by step procedure, but an overview of the experiment including controls and how you would “work up” the data to answer your question.

A student ran the following reaction in the laboratory at 610 K:

CO(g) + Cl2(g) COCl2(g)

When she introduced 0.183 moles of CO(g) and 0.211 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.72×10-2 M.  

Calculate the equilibrium constant, Kc, she obtained for this reaction.

2.A student ran the following reaction in the laboratory at 546 K:

COCl2(g) CO(g) + Cl2(g)  

When she introduced 0.854 moles of COCl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 0.817 M.  

Calculate the equilibrium constant, Kc, she obtained for this reaction.

3. Consider the following reaction:

COCl2(g) CO(g) + Cl2(g)

If 6.56×10-3 moles of COCl2, 0.377 moles of CO, and 0.372 moles of Cl2 are at equilibrium in a 16.9 L container at 772 K, the value of the equilibrium constant, Kp, is

What is the pH of a buffer solution prepared by adding 15.0 g of ammonia chloide to 5.00 L of 0.200 M ammonia? Ka of ammonium is 5.8 x 10^-10

2) What is the pH of the buffer after 90.0mL of 2.00 M HCl are added?

3) What is the pH of the buffer if 15.00 g of NaOH is added to the original buffer solution?

40.00 mL of a 0.1000 M carbonic acid (H₂CO₃) was titrated with 0.2000 M sodium hydroxide.

carbonic acid pka1:6.35 pka2:10.33

1.Calculate the volume of sodium hydroxide required to reach the first equivalence point.

2.Calculate the volume of sodium hydroxide required to reach the second equivalence point.

3.Write the balanced acid-base reaction and calculate the pH before the addition of sodium hydroxide.

4.Write the balanced acid-base reaction and calculate the pH after the addition of 12.00 mL of sodium hydroxide

5.Write the balanced acid-base reaction and calculate the pH after the addition of 20.00 mL of sodium hydroxide

6. Write the balanced acid-base reaction and calculate the pH after the addition of 30.00 mL of sodium hydroxide

7.Write the balanced acid-base reaction and calculate the pH after the addition of 40.00 mL of sodium hydroxide

8.Write the balanced acid-base reaction (paper only) and calculate the pH after the addition of 44.00 mL of sodium hydroxide

to a 100.0 mL volumetric flask are added 1.00 mL volumes of three solutions: .0100 M AgNO3, .205 M NaBr, and .100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigerously. What mass of AgBr would precipitate from this mixture? Hint: The Ksp of AgBr is 5.4 x 10-13 and the Kf of Ag(CN)2- is 1.0 x 10^21