An electroplating solution is made up of nickel (II) sulfate. How much time (in

Question

An electroplating solution is made up of nickel (II) sulfate. How much time (in minutes or seconds) would it take to deposit 0.500 g of metallic nickel on a custom car part using a current of 3.00 A? For the reaction: Zn^2^+ (aq) + Sn(s) rightarrow Zn(s) + Sn^2+ (aq) E degree = -0.62 V. Calculate the cell potential I f [Zn^2+] = 1.0 Times 10^-4 M and [Sn^2+] = 0.2 M. +0.52 V -0.52 V -0.72 V +0.72 V -0.62 V If Delta G degree of the following reaction is -114 kJ/mol what is E degree (F = 96, 500 C mol^-1)? A^3^+ (aq) + 3B (s) rightarrow A(s) + 3B^+(aq) -0.09 V -0.39 V +0.00039 V +0.09V +0.39 V Determine Delta S degree for the reaction SO_3(g) + H_2O (l) rightarrow H_2SO_4(l) 1343.2 J/K middot mol -29.4 J/K middot mol 29.4 J/K middot mol -169.2 J/K middot mol 169.2 J/K middot mol The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ mol at 25 degree C. Find K_p for the reaction H_2(g) + l_2(s) doubleheadarrow 2HI(g) at this temperature. 7100 0.35 7.0 1.0 2.4 The value of E_cell degree for the reaction 2Cr^3+ (aq) + 6Hg(l) rightarrow 2Cr(s) + 3H_2^2+ (aq) is 1.59 V. Calculate Delta G degree for the reaction. -307 kJ -921 kJ -767 kJ -460 kJ None of these choices is correct.

Explanation / Answer

Solved the first four problems, post one more question to get the remaining answers

8)

Molar mass of Nickel = 58.6 gm/mol

Number of moles of Nickel = Mass/molar mass = 0.500/58.6 = 0.0085324 moles

1 mole of Ni(+2) requires 96500C X 2 = 193000C of charge, which is equal to F * (Charge on the metal)

Hence the charge required for 0.0085324 moles = 0.0085324 * 193000 = 1646.75C

Q = I * t

1646.75 = 3 * t

t = 548.91 seconds = 9.148 minutes

9)

Ecell = Eocell - 0.0592/2 * log(K)

K = [Sn+2]/[Zn+2] = 0.2/(1 * 10^(-4)) = 2 * 10^3 = 2000

Ecell = -0.62 - 0.0296log(2000)

=> -0.62 - 0.0977

=> -0.7177

Hence the correct answer is Option C

10) Change in electrons = change in oxidation number of A

=> 3 - 0 = 3

Delta G = -nFEcell

-114 * 10^3 = -3 * 96500 * Ecell

Ecell = 0.3937V

Hence the correct answer is Option E

11)

Delta S(rxn) = DeltaS(products) - DeltaS(reactants)

=> DeltaS(H2SO4(l)) - DeltaS(SO3(g)) - DeltaS(H2O(l))

=> 156.9 - 69.9 - 256.2

=> -169.2 J/mol

Hence the correct answer is Option D

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