Question

Calculate the Delta G for the following reaction at 25 degrees Celcius

3Co^+2 (aq) + 2Al(s) <-> 3Co(s)+2Al^+3(aq)

Answer #1

oxidation :

Al -----------------------> Al+3 + 3e- , Eo = -1.66 V

reduction:

Co+2 + 2e- -----------------------> Co + 2e- , Eo = -0.28 V

Eocell = Eo reduction - Eo oxidation

= -0.28 - (-1.66)

= 1.38 V

n = number of electrons transfered

Delta G = -n F Eo

= - 6 x 96485 x 1.38 x 10^-3 kJ

= -799 kJ /mol

**Delta G = - 799 kJ /mol**

Calculate Delta G° for the following reaction at 25°C:
3Zn2+(aq) + 2Al (s) = 3Zn
(s) + 2Al 3+(aq)
Delta G° = ? kJ/mol

Given that: 2Al(s) + 3/2O2(g) -->
Al2O3(s) Delta H degrees rxn =-1601kJ/mol
and 2Fe(s) + 3/2O2(g) -->
Fe2O3(s) Delta H degrees rxn =-821kJ/mol
Calculate the standard enthalpy change for the following
reaction: 2Al(s) + Fe2O3(s) --> 2Fe(s) +
Al2O3(s)
Answer in scientific notation

Consider the following reaction CaSO4 (s) ------- Ca +2 (aq) +
SO4 -2 (aq)
A. Calculate delta H
B. Calculate delta S
C. Calculate delta G at 25 C

Calculate the delta H degrees reaction for the following
reaction:
2Ni(s) + 2S(s) +3O2 (g) -> 2NiSO3(s)
from the following info:
NiSO3(s) -> NiO(s) + SO2(g) delta H=156kJ
S(s) + O2(g) -> SO2(g) delta H= -297
Ni(s) + 1/2O2(g) -> NiO(s) delta H = -241

Calculate the Delta G Reaction at 318 K under the conditions
shown below for the following reaction. Fe2O3 (s) + 3CO (g) -->
2 Fe(s) + 3CO2 (g) Delta G= -28.0kJ

Calculate Eo, E, and delta G for the following cell
reaction
3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s) where [Cr3+] = 0.090 M
and [Zn2+] = 0.0095 M
I found Eo to be 0.02 V
I'm having trouble finding E and delta G

1. Consider the following reaction: 2Al(s) + 6HCl(aq) >
2AlCl3(aq) +3H2(g)
A 1.0792-g piece of aluminum reacted completely in 20.0 s. The
rate of formation of hydrogen gas is:
A) 6.05 * 10-3 g/s
B) 2.00 * 10-3 g/s
C) 1.56 * 10-3 g/s
D) 3.15 * 10-3 g/s

Calculate the enthalpy of reaction for the following reaction:
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol
ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5
kJ/mol

A 2.0L equilibrium mixture of the reaction
2A(s)+B(g)<=>2C(g) at 25 degrees celcius was found to contain
0.30 moles of A, 0.50 moles of B and 0.60 moles of C. At 200
degrees celsius, the concentration of C is found to be twice the
concentration of B.
a) What is the Kp and Kc of this reaction at 25 degrees
celsius?
b) What is the Kc at 200 degrees celsius?

Calculate the following for the combustion of 1.00 mole of
C6H6(L) at 25 degrees celcius, delta Hf, C6H6 (L) = 49.04
kJ/mol.
a) The heat flow at a constant pressure of 1.00 atm.
b) The heat flow at a constant volume
c) The work at a constant pressure of 1.00 atm
d) The work at a constant volume

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