Calculate δg° for the following reaction from the equilibrium constant at the temperature given. hf(aq)+h2o(l)⟶h3o+(aq)+f−(aq),t=25° c, k=7.2×10−4

17.93 kJ

Explanation:

The relation between standard Gibbs energy and equilibrium reaction is shown below as:

R is Gas constant having value = 0.008314 kJ / K mol  

Given For the reaction:-

temperature, T =

Applying in the above equation as:-

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.

i think it's letter a.