Question

In: Chemistry

1. Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of...

1. Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-6 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10–14.
A) A precipitate forms because Qc > Ksp.
B) A precipitate forms because Qc < Ksp.

C) No precipitate forms because Qc < Ksp.

D) No precipitate forms because Qc = Ksp.

E) No precipitate forms because Qc > Ksp.

2. For which of the following reactions is ∆S° > 0 at 25°C?

A) 2H2(g) + O2(g) → 2H2O(g)
B) 2ClBr(g) → Cl2(g) + Br2(g)
C) I2(g) → I2(s)

D) 2NO(g) + O2(g) → 2NO2(g)

E) NH4HS(s) → NH3(g) + H2S(g

3. What is E of the following cell reaction at 25°C? Cu(s) | Cu2+(0.017 M) || Ag(s), (Ag+ = 0.18M)

E°cell = 0.460 V.

A) 0.468V

B) 0.282 V

C) 0.460 V

D) 0.490 V

E) 0.479V

Solutions

Expert Solution

Q1 Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-6 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10–14.

Solution :-

Using the given concentration values lets calculate the Qc

Qc equation is as follows

Qc=[Fe^3+][IO3^-]3

Lets put the values in the formula after adding the solution total volume will become 100 ml therefore the initial concentrations will halved.

[Fe^3+] = 2.0E-4 / 2 = 1.0E-4 M

[IO3^-] = 2.0E-6 / 2 = 1.0E-6 M

Qc = [1.0E-4 ] [1.0E-6]2

Qc = 1E-16

Therefore Qc is smaller than Kc means reaction will proceed in forward direction.

Therefore correct answer is

No precipitate forms because Qc < Ksp.

Q2 solution

For the reaction

NH4HS(s) → NH3(g) + H2S(g)

Delta S > 0at 25 c

Because here solid is changing to the gases.Gases have the greatest entropy than liquid and solid.

Therefore the reaction shown in the option E will have entropy greater than 0

Q3 solution :-

Cu(s) | Cu2+(0.017 M) || Ag(s), (Ag+ = 0.18M)                       E°cell = 0.460 V.

Formula to calculate the E of cell is as follows

E cell = Eo cell – (0.0592/n)logQ

Where log Q = [product ]/[reactant]

N=number of electrons transferred.

Lets put the values in the formula

E = 0.460 V – (0.0592/2)log [0.017/0.18]

E= 0.460 V – (-0.0303)

E= 0.490 V

Therefore correct answer is option ‘D’


Related Solutions

A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x...
A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x 10-3 M KSCN, and 1.00 mL of distilled water and finds that in the equilibrium mixture, the concentration of FeSCN2+ is 1.31 x 10-4 M. The equation describing the equilibrium is Fe3+ (aq) + SCN- (aq) →← →← FeSCN2+ (aq) Calculate the concentration of FeSCN2+ at equilibrium. Include appropriate significant figures and units in your response. Example input: 1.31x10^-4 M.
A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x...
A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x 10‐3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.40 x 10‐4 M. What is the initial concentration in solution of the Fe+3 and SCN‐? What is the equilibrium constant for the reaction? What happened to the K+ and the NO3‐ ions in this solution?
20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and...
20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and 12.00 mL of water. The equalibrium molarity of Fe(SCN)2+ is found to be 6.82E-5 M. If the reaction proceeds as shown below, what is the equilibrium molarity of Fe3+ and SCN-?    Fe3+(aq) + 2 SCN-(aq) Fe(SCN)2+(aq) I have the answers (they are correct according to my online homework), but need to know how to get them. Thank you! The correct answeers are: Fe =...
10.00 mL of 3.48E-3 M Fe(NO3)3 is mixed with 4.00 mL of 2.84E-3 M KSCN and...
10.00 mL of 3.48E-3 M Fe(NO3)3 is mixed with 4.00 mL of 2.84E-3 M KSCN and 6.00 mL of water. The equalibrium molarity of FeSCN2+ is found to be 8.70E-5 M. If the reaction proceeds as shown below, what is the equilibrium molarity of Fe3+ and SCN-? Fe3+(aq) + SCN-(aq) FeSCN2+(aq) Equilibrium Concentration Fe3+ ____________ Equilibrium Concentration SCN- ____________
Calculate pBa when 50.00 mL of 0.100 M EDTA is added to 50.00 mL of 0.100...
Calculate pBa when 50.00 mL of 0.100 M EDTA is added to 50.00 mL of 0.100 M Ba2+. For the buffered pH of 10, the fraction of EDTA in its fully deprotonated form is 0.30. Kf = 7.59 x 107 for BaY2-. a) 7.36 b) 7.88 c) 1.30 d) 4.33
Suppose 50.00 mL of 0.300 M HCl is added to an acetate buffer prepared by dissolving...
Suppose 50.00 mL of 0.300 M HCl is added to an acetate buffer prepared by dissolving 0.100 mol of acetic acid and 0.110 mol of sodium acetate in 0.100 L of solution. What are the initial and final pH values? What would be the pH if the same amount of HCl solution were added to 170 mL of pure water?
When 100 mL each of 2.0 × 10-4 M Ca2+ and 2.0 × 10-2 M F-...
When 100 mL each of 2.0 × 10-4 M Ca2+ and 2.0 × 10-2 M F- are mixed, what is the remaining Ca2+ ion concentration ? The solubility product constant of CaF2 is 5.3 × 10-9. (Hint: Determine the limiting reactant, the concentration of excess reactant after precipitation, and how the concentration of excess reactant influences the solubility of CaF2).
Calculate the pH of a solution produced during the titration of 50.00 mL of 2.0 M...
Calculate the pH of a solution produced during the titration of 50.00 mL of 2.0 M acetic acid with 1.0 M potassium hydroxide and the following volumes of base added: a) 0.00 mL b) 25.0 mL c) 50.0 mL d) 100.0 mL e) 125.0 mL
Suppose a 500. mL flask is filled with 0.20 mol of NO3 and 2.0 of NO...
Suppose a 500. mL flask is filled with 0.20 mol of NO3 and 2.0 of NO the following reaction becomes possible NO3(g) + NO (g) =2NO2(g) the equilibrium constant K for this reaction is 4.05 at the themperature of the flask .calculate the equilibrium Molarity of NO round to two decimal places final answer in Molarity .
56.0 mL of 2.50 M Fe(NO3)2 is combined with 25.0 mL of 0.0525 M Na2CO3. Ksp...
56.0 mL of 2.50 M Fe(NO3)2 is combined with 25.0 mL of 0.0525 M Na2CO3. Ksp of FeCO3 is 2.1 × 10-11. What mass of FeCO3(s) will be produced? in grams What is the [Fe2+] in the solution final solution? in M What is the [CO32-] in the solution final solution? in M
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT