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sertanlavr [38]
2 years ago
5

T = 409.5 K, P = 1.50 atm: V = ?L

Chemistry
1 answer:
Molodets [167]2 years ago
7 0

Explanation:

T = 409.5 K, P = 1.50 atm: V = 22.4 L The ideal gas law is: PV = nRT where. P = pressure. V = volume n = number of moles.

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Determine the equilibrium constant, Keq, at 25°C for the reaction
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Explanation:

The given chemical reaction is:

2Br^- (aq) + I_2(s)  Br_2(l) + 2I^- (aq)

E^ocell=oxidation potential of anode + reduction potential of cathode\\

The relation between Eo cell and Keq is shown below:

deltaG=-RTlnK_e_q\\delta=-nFE^o cell\\=>nFE^o cell=RTlnK_e_q\\lnK_e_q=\frac{nF}{RT} E^o cell

The value of Eo cell is:

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Oxidation takes place at anode.

Hence,

E^ocell= (-1.07+0.53)V\\=-0.54V

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R=8.314 J.K-1.mol-1

T=298K

Substitute all these values in the above formula:

ln K_e_q=\frac{2mol* 96485 C/mol}{8.314 J.K^-^1.mol^-^1x298K} \\\\lnK_e_q=77.8\\K_e_q=e^7^7^.^8\\=>K_e_q=6.13x10^3^3

Answer:

Keq=6.13x10^33

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What volume (in L) of a 1.25 M
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Answer:

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Explanation:

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Now make the substitution

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Rearrange to make V1 the subject

V1=

\frac{0.838 \times 0.455}{1.25 }  = 0.305

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