Balancing Redox Equations in Acidic or Basic Solutions

In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods. The oxidation number method balances the net increase in oxidation of the substance oxidized with the net decrease in the oxidation number of the substance reduced. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In both methods

H2O(l),OH?(aq), and H+ (aq) may be added to complete the mass balance. Which substances are used depends on the reaction conditions.

Acidic solution

In acidic solution, bromate ion can be used to react with a number of metal ions. One such reaction is

BrO3?(aq)+Sn2+(aq)?Br?(aq)+Sn4+(aq)

Since this reaction takes place in acidic solution,

H2O(l)andH+(aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:

BrO3?(aq)+Sn2+(aq)+ ____ ?Br?(aq)+Sn4+(aq)+ ___

Part A

What are the coefficients of the six species in the balanced equation above? Remember to include coefficients for

H2O(l)andH+(aq)

in the appropriate blanks.

Enter the equation coefficients in order separated by commas (e.g., 2,2,1,4,4,3).

Basic solution

Potassium permanganate,

KMnO4, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction conditions used. In basic solution, the following equation represents the reaction of this ion with a solution containing sodium sulfite:

MnO4?(aq)+SO32?(aq)?MnO2(s)+SO42?(aq)Since this reaction takes place in basic solution,H2O(l)andOH?(aq)

will be shown in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:

MnO4?(aq)+SO32?(aq)+ ____?MnO2(s)+SO42?(aq)+ ___

Part B

What are the coefficients of the six species in the balanced equation above? Remember to include coefficients for

H2O(l)andOH? (aq) in the blanks where appropriate.

Enter the equation coefficients in order separated by commas (e.g., 2,2,1,4,4,3).

At 20

Describe Kinetic Molecular theory

)Describe in sentences and pictures the terms effusion and diffusion. Find, write out and solve one effusion/diffusion problems within or at the back of the gas chapter .

Calculate ΔGo at 25oC for the reaction H2 + I2 D 2HI. Starting with 1.0 atm H2 and 1.0 atm I2, What is ΔG when: 0.1%, 1%, 10%, 50%, 90%, 99%, and 99.9% has reacted.

Suppose you titrated your standard acid (KHP) with the base to be standardized, but added several drops extra of the base (i.e. stopped the titration after the phenolphthalein indicator in the solution turned very pink).

If this calculated value was used to determine the molar mass of the unknown acid, what type of error would you have for the molar mass of the unknown acid? (i.e. would you overestimate or underestimate the molar mass value?) Support your answer by, for every step in the calculation, determining whether the calculated value would be greater or less than it should be.

how to put formulate the question :
Calculate the number of atoms present in 3.752g sample of Pb? 

a) Write the net ionic equations for any reaction that occurs when each of the following salts are dissolved in water (if no reaction occurs, write "NR"):

ammonium nitrate

potassium bromide

cesium formate

b) When does the cation of a salt react with water. Illustrate answer using KBr and NH₄Br:

c) When does the anion of salt react with water. Illustrate answer using KBr and KF:

You dissolve a compound with a molecular mass of 289.49 in a 10-mL volumetric flask. You remove a 1.00-mL aliquot, place it in a 25-mL volumetric flask and dilute it to the mark. The absorbance of this diluted solution at 341 nm was 0.444 in a 1.000-cm cuvet. The molar absorptivity for this compound at 341 nm is ε341 = 6117 M–1 cm–1.

(a) What is the concentration of the compound in the cuvet?

(b) What is the concentration of the compound in the 10-mL flask?

(c) How many milligrams of compound were used to make the 10-mL solution?

Predict whether N₂ is likely to have a relatively high or low boiling point.

Dalton's Law Of Partial Pressure show all calculations!!

a.) Earth's atmosphere consist of 78% N2 and 20% O2, and other gases. What is the partial pressure of N2 and O2 in torr, when atmospheric pressure is 1 atm?

b.) Ammonia is completely decomposed to nitrogen and hydrogen as in question 9b) At the end of the experiement the pressure of the gas mixture is 866 mmHg. Calculate the partial pressures of N2 and H2

11)

What are the coefficients in front of NO₃^-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution:
___ NO₃^-(aq) + ___ Cu(s) → ___ NO(g) + ___ Cu²⁺(aq)?

Select one:

A. 3, 6

B. 2, 6

C. 2, 3

D. 3, 4

12)

The values of ΔH°_f for the three states of benzene are approximately -22 kcal/mol, -11 kcal/mol, and 20kcal/mol. Which is the value for solid benzene?

Select one:

A. -22 kcal/mol

B. 20 kcal/mol

C. -11 kcal/mol

D. cannot be determined without additional information

13)

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl₄(l) from 35.0°C to gaseous CCl₄ 76.8°C (the normal boiling point for CCl₄)? The specific heat of CCl₄(l) is 0.857J/gC its heat of fusion is 3.27kj/mol and its heat of vaporization is 29.82kJ/mol.

Select one:

A. 1.43 kJ

B. 6.28 kJ

C. 5.74 kJ

D. 0.896 kJ

18)

When heated, mercury(II) oxide decomposes into elemental mercury and oxygen:
2 HgO(s) → 2 Hg(l) + O₂(g) ΔH° = 181.6 kJ ΔS° = 216.4 J/K
Estimate the temperature at which HgO should begin to decompose if the partial pressure of O₂(g) is constant at 1.00 atm.

Select one:

A. 840°C

B. -34.8°C

C. 34.8°C

D. 566°C

19)

When 50.0 mL of 0.400 M Ca(NO₃)₂ is added to 50.0 mL of 0.800 M NaF, CaF₂ precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 25.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of calculate the final temperature of the solution.
Ca²⁺(aq) + 2 F^-(aq) → CaF₂(s) ΔH° = -11.5 kJ

Select one:

A. 24.45°C

B. 26.10°C

C. 26.65°C

D. 25.55°C

Physical chemistry

. The osmotic of an aqueous solution at 351 K is 94 kPa and a density of 1,152 g/mL. Calculate the freezing point (in C) of the solution. The Kf for water is 1.86oC/m.

How does pentobarbital, pancuronium bromide, and potassium chloride accomplish cessation of life?

Please include a source(s)!! It is a necessity! Thank you.

If a temperature scale were bassed on the freezing point (5.5 degrees Celsius) and boiling point (80.1 degrees Celsius) of benzene, and the temperature difference between these two points was divided into 50 units called degrees X, what would be the freezing and boiling points of water in degrees X?