Table of contents

1. Introduction to Biochemistry4h 34m
2. Water3h 23m
3. Amino Acids8h 10m
4. Protein Structure10h 4m
5. Protein Techniques14h 5m
6. Enzymes and Enzyme Kinetics13h 38m
7. Enzyme Inhibition and Regulation 8h 42m
8. Protein Function 9h 41m
9. Carbohydrates7h 49m
10. Lipids5h 49m
11. Biological Membranes and Transport 6h 37m
12. Biosignaling9h 45m
Review 1: Nucleic Acids, Lipids, & Membranes2h 47m
Review 2: Biosignaling, Glycolysis, Gluconeogenesis, & PP-Pathway3h 12m
Review 3: Pyruvate & Fatty Acid Oxidation, Citric Acid Cycle, & Glycogen Metabolism2h 26m
Review 4: Amino Acid Oxidation, Oxidative Phosphorylation, & Photophosphorylation1h 48m

1. Introduction to Biochemistry

Entropy

Biochemistry

1. Introduction to Biochemistry

Entropy

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Multiple Choice

Consider a reaction at 100˚C with ΔG = 15 KJ and ΔH = 40 KJ. Calculate the system's change in entropy.

139.13 kJ/K

-13.3 kJ/K

0.15 kJ/K

0.07 kJ/K

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Verified step by step guidance

Start by recalling the Gibbs free energy equation: ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.

Convert the given temperature from Celsius to Kelvin. Since the temperature is given as 100˚C, add 273.15 to convert it to Kelvin: T = 100 + 273.15 = 373.15 K.

Rearrange the Gibbs free energy equation to solve for ΔS: ΔS = (ΔH - ΔG) / T.

Substitute the given values into the rearranged equation: ΔH = 40 KJ, ΔG = 15 KJ, and T = 373.15 K.

Calculate ΔS using the substituted values to find the change in entropy of the system.