Which of the reactions are spontaneous (favorable)? a. dhap↽−−⇀glyceraldehyde-3-phosphateδ =3.8 kj/mol b. c2h4+h2−→−−rh(i)c2h6δ=−150.97 kj/mol c. glutamate+nad++h2o⟶nh+4+α-ketogluta rate+nadh+h+δ=3.7 kcal/mol d. c6h13o9p+atp⟶c6h14o12p2+adpδ=−14.2 kj/mol e. l -malate+nad+⟶oxaloacetate+nadh+h+δ= 29.7 kj/mol

The spontaneous reactions are:

B. ; ΔG= −150.97 kJ/mol  

D. C₆H₁₃O₉P + ATP ⟶ C₆H₁₄O₁₂P₂ + ADP; ΔG = −14.2 kJ/mol  

Explanation:  

Gibbs free energy , denoted by ΔG, is the quantitative measure of the favorability or spontaneity of a given process or chemical reaction that is carried out at constant temperature (T) and pressure (P).

Therefore, Gibbs free energy in J: ΔG = ΔH - TΔS

Here, ΔH is the change in enthalpy and ΔS is the change in the entropy

For a given chemical reaction to be spontaneous or favorable, ΔG should be negative (ΔG < 0).

A. DHAP ⇌ glyceraldehyde-3-phosphate ; ΔG = 3.8 kJ/mol  

The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.

B. ; ΔG= −150.97 kJ/mol  

 The value of ΔG is negative (ΔG < 0). Therefore, this reaction is spontaneous.

C. glutamate + NAD⁺ + H₂O ⟶ NH⁴⁺ +α-ketoglutarate + NADH + H⁺ ; ΔG = 3.7 kcal/mol  

The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.

D. C₆H₁₃O₉P + ATP ⟶ C₆H₁₄O₁₂P₂ + ADP; ΔG = −14.2 kJ/mol  

 The value of ΔG is negative (ΔG < 0). Therefore, this reaction is spontaneous.

E. L -malate + NAD⁺ ⟶ oxaloacetate + NADH + H⁺; ΔG = 29.7 kJ/mol

The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.