The standard free energy change for a reaction can be calculated using the equation
where n is the number of electrons transferred f is faraday\'s constant, 96.5 kj·mol−1·v−1, and δ e ∘ \' is the change reduction potential
for each of the following reactions, determine the number of electrons transferred (n) and calculate standard free energy ( δ g ∘ ′ ).

a) half-reactions: fumarate2- + 2h+ < --> succinate2-
coqh2 < --> coq + 2h+
overall reaction: fumarate2- + coqh2 < --> succinate2- + coq ( δg∘ ′ ) = -0.009v
n=( δ g ∘ ′ ) = kj*mol-1

b) half-reactions: cytochrome c1(fe2+) < --> cytochrome c1 (fe3+)
cytochrome c (fe3+) < --> cytochrome c (fe2+)
overall reaction: cyt c1 (fe2+) + cyt c (fe3+) < --> cyt c1 (fe3+) + cyt c (fe2+)( δe∘ ′ ) = 0.02v
n= ( δ g ∘ ′ )' = kj*mol-1

1. suppose a reaction mixture, when diluted with water, afforded 300 ml of an aqueous solution of 30 g of the reaction product malononitrile [ch2(cn)2], which is to be isolated by extraction with ether. the solubility of malononitrile in ether at room temperature is 20.0 g/100 ml, and in water is 13.3 g/100 ml. what weight of malononitrile would be recovered by extraction with (a) three 100-ml portions of ether and (b) one 300-ml portion of ether? suggestion: for each extraction, let x equal the weight extracted into the ether layer. in part (a), the concentration in the ether layer is x/100 and in the water layer is (30 x)/300; the ratio of these quantities is equal to k 20/13.3.

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl+4h2o enter the elemental symbol. view available hint(s) is reduced

The atoms of a solid aluminum can are close together, vibrating in a rigid structure. if the can is warmed up on a hot plate, what happens to the atoms?