For a certain process at 355 K, deltaG = -11.8 kJ and deltaH = -9.2 kJ. Therefore, deltaS for the process is ______ J/K mol
Added by Joshua R.
Close
Step 1
8 kJ - ΔH = -92 kJ Converting to J: - ΔG = -11.8 kJ * 10^3 J/kJ = -11,800 J - ΔH = -92 kJ * 10^3 J/kJ = -92,000 J Show more…
Show all steps
Your feedback will help us improve your experience
Suman K and 69 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
Consider the following reaction occurring at 298K: ΔG°' = -16.7 kJ/mol, calculate K'eq
Adi S.
For a certain process at 355K, ΔG = -10.1 kJ and ΔH = -9.2 kJ. Therefore, ΔS for the process is: 0 2.5 J/K mol -2.5 J/K mol -25.9 J/K mol 25.9 J/K mol
Narayan H.
$$ \begin{aligned} &\text { Calculate the value of } \Delta G \text { at } 700 \mathrm{~K} \text { for the reaction } n X \longrightarrow m B .^{-1}\\ &\text { Given that value of } \Delta H=-113 \mathrm{~kJ} \mathrm{~mol}^{-1} \text { and } \Delta S=-145 \mathrm{JK} \mathrm{mol}^{-1} \text { . } \end{aligned} $$
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD