The standard reduction potential, e′°, of any redox pair is defined for the half-cell reaction: oxidizing agent + n electrons → reducing agent the e′° values for the nad+/nadh and pyruvate/lactate conjugate redox pairs are −0.32 v and −0.19 v, respectively. (a) which redox pair has the greater tendency to lose electrons? explain. (b) which pair is the stronger oxidizing agent? explain. (c) beginning with 1 m concentrations of each reactant and product at ph 7 and 25 °c, in which direction will the following reaction proceed? pyruvate + nadh + h+ \rightleftharpoons lactate + nad+d) what is the standard free energy change (? g’°) for the conversion of pyruvate to lactate? e) what is the equilibrium constant (k’eq) for this reaction?

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.

the answers would be

the first one and the second one

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2