If ?H = -80.0 kJ and ?S = -0.400 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
Added by Nicholas G.
Step 1
The formula for ΔG is: ΔG = ΔH - TΔS We are given ΔH = -80.0 kJ and ΔS = -0.400 kJ/K. We want to find the temperature (T) at which the reaction becomes spontaneous, which means ΔG < 0. -80.0 kJ - T(-0.400 kJ/K) < 0 Now, we can solve for T: Show more…
Show all steps
Your feedback will help us improve your experience
Nicholas Mogoi and 82 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
If ΔH = -80.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
Adi S.
If ΔH= -60.0 kJ and ΔS = -0.200 kJ/K, the reaction is spontaneous below a certain temperature. Calculate that temperature.
David C.
If ΔH = -70.0 kJ and ΔS = -0.200 kJ/K, the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
Amita P.
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