Question

Consider the reaction

Mg(s)+Fe2+(aq)?Mg2+(aq)+Fe(s) at 53?C , where [Fe2+]= 3.80M and [Mg2+]= 0.310M .

a)What is the value for the reaction quotient, Q, for the cell?

b)What is the value for the temperature, T, in kelvins?

c)What is the value for n?

Express your answer as an integer and include the appropriate units (i.e. enter mol for moles).

Answer 1

Given, [Fe2+] = 3.80M and [Mg2+] = 0.310M

The given cell reaction is

Mg(s) + Fe2+(aq) -------------------> Mg2+(aq) + Fe(s)

(a) The Q value for the above cell reaction can be calculated as

Q = [Product] / [reactant] = [Mg2+] / [Fe2+]   = 0.310 M / 3.80 M = 0.0816   (answer)

(b) Temperature, T = 53 degC = 53 +273 = 326 K. (answer)

(c) Here Mg(s) loses 2 electrons to oxidise to Mg²⁺ (aq), and Fe²⁺ (aq) gains these 2 electrons to reduce to Fe(s).

Hence n value for the above reaction is 2 (answer)