the formula for delta G = - 2.303 RT Log Keq
Ans. 1. Rearranging the above equation, we get -
Keq = 10^ -delta G/1.36
Keq = 10^ - 1.8 / 1.36
Keq = 10^ 1.32
Keq = 20.89 or 20.9
so a product : reactant ratio of 20.9 : 1 must be maintained in order to drive the reaction forward.
Ans. 2 delta G = - 2.303 RT Log Keq
= - 1.36 log 02818
- 1.36 x 3.45
= - 4.6 Kcal
Solve using Log not LN Problems and Essays For the reaction dihydroxyacetone phosphate glyceraldehyde 3-phosphate ΔG"=1.8...
For the aqueous reaction dihydroxyacetone phosphate is the reactant and glyceraldehyde 3 phosphate is the product. dihydroxyacetone phosphate↽−−⇀glyceraldehyde−3−phosphate dihydroxyacetone phosphate ↽ − − ⇀ glyceraldehyde − 3 − phosphate the standard change in Gibbs free energy is Δ?°′=7.53 kJ/mol Δ G ° ′ = 7.53 kJ/mol . Calculate Δ? Δ G for this reaction at 298 K 298 K when [dihydroxyacetone phosphate]=0.100 M [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate]=0.00400 M [glyceraldehyde-3-phosphate] = 0.00400 M .
For the aqueous reaction dihydroxyacetone phosphate is the reactant and glyceraldehyde 3 phosphate is the product. dihydroxyacetone phosphate − ⇀ ↽ − glyceraldehyde − 3 − phosphate the standard change in Gibbs free energy is Δ G ° ' = 7.53 kJ/mol . Calculate Δ G for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00300 M .
please help. Juction reaction In one step of glycolysis, glyceraldehyde 3-phosphate is oxidized by NAD+ to yield 3-phosphoglycerate and NADH. 1) Consider that reaction, in the direction written. Which chemical(s) is/are) losing electrons, and which chemical(s) is(are) gaining electrons? It's best to answer this in a clear complete sentence! 2) Calculate the standard reduction potential for this reaction. Show a reasonable amount of your work (you don't need to show every step in a calculation, but at least show your...