Given the following standard reduction potentials, answer the following question

Question

Given the following standard reduction potentials, answer the following question. Fe^3+(aq) + 2e^- rightarrow Fe^2+(aq) + .771 Sn^4+(aq) + 2e^- rightarrow Sn^2+(aq) + .154 The standard cell potential (E degree cell) for the voltaic cell based on the reaction below is ______ V. Sn^2+(aq) + 2Fe^3+ (aq) rightarrow 2 Fe^2+(aq) + Sn^4+(aq) a. +.46 b. +.617 c. +1.39 d. -.46 e. +1.21 For the reaction C_2H_5(g) rightarrow C_2H_4(g) + H_2(g) Delta H^o is +137 kJ/mol and Delta S^o is + 120 J/mol. This reaction is _______. a. spontaneous at all temperatures b. spontaneous only at high temperatures c. spontaneous only at low temperatures d. nonspontaneous at all temperatures e. unreliable Consider the following chemical reaction H_2(g) + l_2(g) rightarrow 2 HI(g) At equilibrium in a particular experiment, the concentrations of H_2, l_2, and HI were .15 M, .033M, and .55M, respectively. The value for the K_eq for this reaction is ______. a. 23 b. 111 c. 9.0 times 10^-3 d. 6.1 e. 61 The data in the table below were obtained for the reaction: A + B rightarrow P The rate law is R = k [A]^k[B]^y where x, y equal _____. a. 1, 0 b. 2, 1 d. 2, 0 e. 0, 2

Explanation / Answer

1)

from data table:

Eo(Sn4+/Sn2+) = 0.154 V

Eo(Fe3+/Fe2+) = 0.771 V

As per given reaction/cell notation,

cathode is (Fe3+/Fe2+)

anode is (Sn4+/Sn2+)

Eocell = Eocathode - Eoanode

= (0.771) - (0.154)

= 0.617 V

Answer: b

2)

G = H - T*S

for spontaneous reaction, G should be negative

here both H and S are positive, so G will be negative at higher T

So, it will be spontaneous at high temperature

Answer: b

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