A gaseous reaction occurs at a constant 0.878 atm and released 49.01 kJ of heat, resulting in a volume increase of 23.6 L. What is the total energy for this process ?
Added by Dan
Step 1
We know that 1 atm = 101325 Pa. So, 0.878 atm = 0.878 * 101325 = 89144.55 Pa. Show more…
Show all steps
Your feedback will help us improve your experience
Ankur S and 65 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
An ideal gas undergoes a reversible isothermal expansion at $132^{\circ} \mathrm{C}$. The entropy of the gas increases by $46.2 \mathrm{~J} / \mathrm{K}$. How much heat is absorbed?
A system undergoes an increase in internal energy of 93.3 J, while the gas in the system is compressed from 561 mL to 228 mL under a constant external pressure of 3.6 atm. What is the heat change of the system? 101.3 J = 1 L/atm
Urvashi A.
What is the enthalpy change $(\Delta H)$ for a reaction at a constant pressure of 1.00 atm if the internal energy change $(\Delta E)$ is 44.0 $\mathrm{kJ}$ and the volume increase is 14.0 $\mathrm{L}$ ? $(1 \mathrm{L} \cdot \mathrm{atm}=101.325 \mathrm{J} .)$
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