Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possible reactions is shown here. Calculate ΔG° and K p for this reaction at 25 °C and comment on the spontaneity of the reaction. 3 NO2(g) + H2O(l )→ 2 HNO3(aq) + NO(g)

Video transcript

Hi everyone here we have a question asking what are the free energy? And the constant for the reaction at 25 degrees Celsius, sulfur fluoride gasses plus two water forms sulfate gasses plus four Hydrofluoric acid, Aquarius. And is the reaction spontaneous? So first we need to calculate our free energy. So our free energy equals the free energy of our product minus the free energy of our reactant. So our free energy eat balls. One more of sulfate times negative. 300. plus four moles of Hydrofluoric acid times 200 negative 278. minus one more of sulfur. Full ride times negative, plus two moles of water times negative 237. and that equals negative 0.6 kg jewels. Now we need to calculate R. K. So our free energy of our reaction equals the negative gas constant times our temperature times the natural log of K. So K. Equals E. To the change negative change in free energy divided by r. Gas constant times our temperature. So that equals E. To the negative negative 0.6 killed rules, times one times 10 to the third jewels per one. Kill a jewel times 8. times 298.15 kelvin and that equals 3. times 10 to the 52nd power. So now for our spontaneity if the change in energy is less than zero, the reaction is spontaneous. If the change in reaction equals zero, the reaction is at equilibrium. If the change is greater than zero, the reaction is non spontaneous, our change in our reaction is less than zero, and K is greater than one, which means it is spontaneous. So our change in energy equals 300.1, probably r k equals 3. times 10 to the 52. And our reaction is spontaneous. So these are our final answers. Thank you for watching. Bye.