Calculate ΔG (in kJ/mol) of the reaction of molecular oxygen and carbon monoxide to produce carbon dioxide. The reaction occurs at 25°C. ΔH = -566 kJ/mol, ΔS = -173 J/K. Based on the result, determine the spontaneity of the reaction.

First we need to write down the chemical equation and balance it: O2 + 2CO -> 2CO2 Given the data, we can calculate ΔG using the following formula: ΔG = ΔH - TΔS However, before we plug in the numbers, we need to make sure that all data are given in correct units: We have to convert temperature into Kelvins: T = 25 + 273 = 298 K The entropy change (ΔS) is given in J/K, but the enthalpy change (ΔH) is given in kJ/mol. Therefore, we have to convert ΔH into J/mol or ΔS into kJ/K. Since the question is asking for ΔG in kJ/mol, it would be sensible to convert ΔS into kJ/K: ΔS = -0.173 kJ/mol Now we can use the formula to calculate ΔG: ΔG = ΔH - TΔSΔG = -566 - 298*(-0.173) ΔG = -514 kJ/mol Given that ΔG is negative, the reaction is exergonic, that is it occurs spontaneously at 25°C.

KM
Answered by Katerina M. Chemistry tutor

4378 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

What does the Maxwell-Boltzmann distribution illustrate?


Why in a strong acid and strong bases reaction, a drop of acid added would not change its PH dramatically but has a big drop near the equivalent point?


Explain how successive ionization energies account for the existence of three main energy levels in the sodium atom.


Why does the atomic radius of an atom decrease as you go across a period?


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning