Question
You remember that $\Delta G^{\circ}$ is related to $R T \ln (K)$ but cannot remember if it's $R T \ln (K)$ or $-R T \ln (K) .$ Realizing what $\Delta G^{\circ}$ and $K$ mean, how can you figure out the correct sign?
Step 1
We know that ΔG° is the standard Gibbs free energy change, which determines the spontaneity of a reaction under standard conditions. If ΔG° is negative, the reaction is spontaneous; if ΔG° is positive, the reaction is non-spontaneous. Show more…
Show all steps
Your feedback will help us improve your experience
Sam Limsuwannarot and 58 other Chemistry 102 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
The equation $\Delta G^{\circ}=-R T \ln K$ relates the value of $K_{\mathrm{p}},$ not $K_{c},$ to $\Delta G^{*}$ for gas-phase reactions. Explain why.
Derive the following equation $\Delta G=R T \ln (Q / K)$ where $Q$ is the reaction quotient and describe how you would use it to predict the spontaneity of a reaction.
Transcript
600,000+
Students learning Chemistry with Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD
