At what temperature (in k) does a reaction start/stop being spontaneous under standard conditions if the reaction has a δh°rxn = +133. 3 kj/mol and δs°rxn = +121. 6 j/(mol∙k)?

A spontaneous reaction is the one that takes place without giving extra efforts like heating or giving energy.. Whereas, a non-spontaneous reaction needs some sort of external help like adding up of a catalyst or heating the solution.

What is the main condition for a reaction to be spontaneous?

For a spontaneous reaction, ∆G . Change in Gibbs free energy should always be negative.

[tex]\Delta {\rm{G= \Delta {\rm{H - T}}\Delta {\rm{S < 0}}[/tex]

Now for the given reaction, Δ[tex]H^0 = +133.3\ kJ/mol = 133.3 *10^3\ J/mol[/tex] and Δ[tex]S^0 = +121.6\ J/mol.K[/tex] Thus, applying the condition of spontaneous reaction,

[tex](133.3 *10^3\ J/mol) - T (121.6 J/mol.K) < 0\\(133.3 *10^3\ J/mol) < T (121.6 J/mol.K) \\T > \frac{133.3 *10^3\ J/mol}{121.6 J/mol.K} \\T > 1096.2 K[/tex]

Hence, at temperature 1096.2 K, the given reaction start being spontaneous.

To learn more about spontaneous reactions, visit:

https://brainly.com/question/11941609

#SPJ4