Most ions tend to be D. Salts. Hope this helps!
Answer;
Yes; this reaction be spontaneous if coupled with the hydrolysis of ATP.
Explanation;
The reaction converting glycerol to glycerol-3-phosphate (energetically unfavorable) can be coupled with the conversion of ATP to ADP (energetically favorable):
Glycerol + HPO42 ⟶glycerol-3-phosphate+H2O
ATP + H2O⟶ ADP + HPO42− + H+
Answer:phosphates are insoluble in water
Explanation:
Answer:
7.28 mol
Explanation:
2 NaOH + H₂SO₄ = 2 H₂O + Na₂SO₄ -------------------(1)
mole fraction for the reaction is;
2 : 1 = 2 : 1
Number of moles of H₂SO₄ = 7.28 mol
1 mol of H₂SO₄ shall form 1 mole of Na₂SO₄
therefore,
7.28 mol of H₂SO₄ shall form 7.28 mole of Na₂SO₄
We cannot solve this problem without using empirical data. These reactions have already been experimented by scientists. The standard Gibb's free energy, ΔG°, (occurring in standard temperature of 298 Kelvin) are already reported in various literature. These are the known ΔG° for the appropriate reactions.
<span>glucose-1-phosphate⟶glucose-6-phosphate ΔG∘=−7.28 kJ/mol
fructose-6-phosphate⟶glucose-6-phosphate ΔG∘=−1.67 kJ/mol
</span>
Therefore, the reaction is a two-step process wherein glucose-6-phosphate is the intermediate product.
glucose-1-phosphate⟶glucose-6-phosphate⟶fructose-6-phosphate
In this case, you simply add the ΔG°. However, since we need the reverse of the second reaction to end up with the terminal product, fructose-6-phosphate, you'll have to take the opposite sign of ΔG°.
ΔG°,total = −7.28 kJ/mol + 1.67 kJ/mol = -5.61 kJ/mol
Then, the equation to relate ΔG° to the equilibrium constant K is
ΔG° = -RTlnK, where R is the gas constant equal to 0.008317 kJ/mol-K.
-5.61 kJ./mol = -(0.008317 kJ/mol-K)(298 K)(lnK)
lnK = 2.2635
K = e^2.2635
K = 9.62
