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pashok25 [27]
3 years ago
8

Consider the reaction between ozone and a metal cation, m2+, to form the metal oxide, mo2, and dioxygen: o3 + m2+(aq) + h2o(l) →

o2(g) + mo2(s) + 2 h+ for which eocell = 0.44. given that eored of ozone is 2.07 v, calculate eored of mo2.
Chemistry
2 answers:
Mandarinka [93]3 years ago
5 0
O3 + M2+(aq) + H2O(l) => O2(g) + MO2(s) + 2 H+
Eo(cell) = Eo(O3/O2) - Eo(MO2/M2+)
0.44 = 2.07 - Eo(MO2/M2+)
Eo(MO2/M2+) = 1.59 V
Phoenix [80]3 years ago
5 0

Answer:

1.63 V

Explanation:

Let's consider the following redox reaction.

O₃(g) + M²⁺(aq) + H₂O(l) → O₂(g) + MO₂(s) + 2 H⁺(aq)

We can identify both half-reactions.

Reduction (cathode): O₃(g) + 2 H⁺(aq) + 2 e⁻ → O₂(g) + H₂O(l)  E°red = 2.07 V

Oxidation (anode): M²⁺(aq) + 2 H₂O(l)  → MO₂(s) + 4 H⁺(aq) + 2 e⁻ E°red = ?

The standard cell potential (E°cell) is the difference between the standard reduction potential of the cathode and the standard reduction potential of the anode.

E°cell = E°red, cat - E°red, an

0.44 V = 2.07 V - E°red, an

E°red, an = 1.63 V

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Pressure is directly proportional to the kelvin temperature. The equation used here is:

P_1T_2=P_2T_1

Where, T_1 and T_2 are initial and final temperatures, P_1 and P_2 are initial and final pressures.

T_1 = 20.3 + 273.15 = 293.45 K

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P_1 = 1.02 atm

T_2  = ?

Let's plug in the values in the equation and solve it for final pressure.

1.02atm(271.15K)=P_2(293.45K)

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5 0
3 years ago
The density of benzene at 15 ∘C is 0.8787 g/mL. Calculate the mass of 0.1200 L of benzene at this temperature.
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Hence, moving from top to bottom along the group the number of shells increases. And with increase in number of shell the atomic or ionic radii increases. As Oxygen is present at the top of the group, therefore, it has the smallest radius due to less number of shells.

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