The standard cell potential (E° cell) of the reaction below is +1.34 V. The value of ΔG° for the reaction is kJ/mol. 3Cu(s)+2MnO−4(aq)+8H+(aq)→3Cu2+ (aq)+2MnO2(s)+4H2O(l)

The standard cell potential (E cell) of the reaction below is +1.34 V. The value of G° for the reaction is kJ/mol.

3Cu(s)+2MnO−4(aq)+8H+(aq)→3Cu2+ (aq)+2MnO2(s)+4H2O(l)

a. -776
b. +259
c. -24.3
d. +776
e. -259

-776 KJ/mol

Explanation:

We must look towards the balanced reaction equation in order to obtain the number of electrons transferred in the redox reaction.

3Cu(s) + 2MnO4^-(aq) + 8H^+(aq)>3Cu2+(aq) + 2MnO2(s) + 4H2O(l)

We can easily see that copper lost six electrons while Manganese gained six electrons hence n=6

ΔG =-nFEcell

Where;

n= 6

F = 96500 C

Ecell=+1.34

ΔG = -(6 * 96500 * 1.34)

ΔG = -776 KJ/mol

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.