Question

1-How many seconds are required to deposit 0.236 grams of manganese metal from a solution that contains Mn2+ ions, if a current of 1.09 A is applied.

2-consider the reaction NH4NO3(aq)N2O(g) + 2H2O(l) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.

Answer 1

1)

the electrolysis expression is:

Mn2+ + 2e- ------> Mn

1 mol of Mn requires 2 mol of electron

1 mol of electron = 96485 C

So,1 mol of Mn requires 192970 C

let us calculate mol of element deposited:

we have below equation to be used:

number of mol, n = mass/molar mass

= 0.236/54.94

= 0.0043 mol

total charge = mol of element deposited * charge required for 1 mol

= 0.0043*192970

= 828.921 C

we have below equation to be used:

time = Q/i

= 828.921/1.09

= 760 seconds

Answer: 760 seconds

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