3. Calculate the free energy change (?G) for the following chemical reaction: ATP ? ADP + Pi The reaction occurs at 293 K, the change in heat (?H) = 19,070 cal, and the change in entropy (?S) = 90 cal/K.
Added by Caleb S.
Close
Step 1
We'll convert calories to joules by multiplying by 4.184 J/cal. ΔH = 19,070 cal × 4.184 J/cal = 79,764.68 J ΔS = 90 cal/K × 4.184 J/cal·K = 376.56 J/K Now, we can use the Gibbs free energy equation: ΔG = ΔH - TΔS where ΔG is the change in free energy, ΔH is Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 96 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Calculate the Gibbs free energy change (ΔG) for the following chemical reaction: ATP → ADP + Pi The reaction occurs at 68ºF, the change in heat (ΔH) = 19,070 calories, and the change in entropy (ΔS) = 90 cal/K.
Christopher N.
If the ΔG' for the hydrolysis of ATP is -30.5 kJ/mol, then calculate the free energy change (ΔG) for this reaction when [ATP] = 2.5 mM; [ADP] = 0.1 mM; [Pi] = 1.0 mM, and T = 37.0°C. Use R = 8.314 J/mol K.
Farhan A.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD