Chemical potential energy
<u>Answer:</u> The Gibbs free energy of the reaction is -445 J/mol.
<u>Explanation:</u>
The chemical equation for the conversion follows:
The expression for of above equation is:
We are given:
[Glyceraldehyde-3-phosphate] = 0.00400 M
[Dihydroxyacetone phosphate] = 0.100 M
Putting values in above equation, we get:
Relation between standard Gibbs free energy and equilibrium constant follows:
where,
= Standard Gibbs free energy = 7.53 kJ/mol = 7530 J/mol (Conversion factor: 1kJ = 1000J)
R = Gas constant =
T = temperature = 298 K
Putting values in above equation, we get:
Hence, the Gibbs free energy of the reaction is -445 J/mol.
The moon phases maybe? Can I see the passage possibly?
The second approach is correct. The other two approaches are not correct because they are incomplete; first approach would have been right IF the 6.0 ppm was MEASURED in hexane. Third approach cannot be right since it calculates moles and grams but not L.
Answer:
<h3>The answer is 7.14 g/mL</h3>
Explanation:
The density of a substance can be found by using the formula
From the question
mass = 10 g
volume = final volume of water - initial volume of water
volume = 52.1 - 50.7 = 1.4 mL
We have
We have the final answer as
<h3>7.14 g/mL</h3>
Hope this helps you