Answered

Discover the answers you need at Westonci.ca, a dynamic Q&A platform where knowledge is shared freely by a community of experts. Join our Q&A platform to connect with experts dedicated to providing accurate answers to your questions in various fields. Discover in-depth answers to your questions from a wide network of professionals on our user-friendly Q&A platform.

For the process 2SO2(g) O2(g) Right arrow. 2SO3(g), Delta. S = –187. 9 J/K and Delta. H = –198. 4 kJ at 297. 0 K are known. What is the entropy of this reaction? Use Delta. G = Delta. H – TDelta. S. –386. 3 J/K –198. 4 kJ/K –187. 9 J/K –139. 3 kJ.

Sagot :

[tex]\rm -187.9 \;J/K[/tex]entropy of the reaction.

Entropy is the amount of heat or temperature inaccessible for the system to work and convert the chemical or thermal energy into mechanical energy.

How to calculate the entropy?

Given,

  • [tex]\rm \Delta S[/tex] = [tex]\rm -187.9 \;J/K[/tex]
  • [tex]\rm \Delta H[/tex] = -198.4 kJ
  • Temperature (T) = 297.0 K

The balanced reaction can be shown as,

[tex]\rm 2SO_{2}(g) + O_{2}(g) \rightarrow 2SO_{3}(g)[/tex]

The Gibbs free energy can be calculated as:

[tex]\rm \Delta G = \Delta H - \rm T\Delta S[/tex]

Here,[tex]\rm \Delta G[/tex] = gibbs free energy, [tex]\rm \Delta H[/tex] = change in enthalpy, T = temperature and [tex]\rm \Delta S[/tex] = change in entropy.

Substituting values in the equation:

[tex]\begin{aligned}\rm \Delta G &= -198400 \;\rm kJ -297 \times (-187.9\;\rm kJ/mol)\\\\\rm \Delta G &= -198400 + 55806.3\\\\\rm \Delta G &= - 142593.7 \;\rm kJ\end{aligned}[/tex]

Therefore, [tex]\rm -187.9 \;J/K[/tex] is the entropy [tex](\rm \Delta S)[/tex] of the reaction.

Learn more about entropy here:

https://brainly.com/question/4617981

Thanks for using our platform. We're always here to provide accurate and up-to-date answers to all your queries. We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Westonci.ca is committed to providing accurate answers. Come back soon for more trustworthy information.