I think we are supposed to use the equation deltaG=-RTlnK
I calculated deltaG= products-reactants but I'm not coming up with the correct answer. Help please
Hey Kathryn! Do you mind sending me a picture of the Appendix IIB? It all depends on what's given there. If not, just send me the values given in the book and the question. Thanks!!
NO= 86.58 O2: 0
Okay, so you are correct, you will be using that equation to solve for K. Remember K is you equilibrium constant, so I rearranged the equation for you in order to solve for K. That's how it should look. Again, you calculate ΔG° by using the formula :
ΔG°rxn = ΔGproducts - ΔGreactants
For your R, you will use the constant R=8.314 J/ mol . K
For your temperature, you must use Kelvin, so add 273 to the 25° C that are given in the problem. You should get T = 298° K.
Just plug all of these values into your calculator and you should get your K. Let me know if this helps!
I'm getting 2.47e12, but it is saying it's the wrong answer.
Here is my work:
2NO: 286.58=173.16 O2:0 2NO2: 251.23=102.46
102.46-173.16=-70.70 converted to J= -70700 J
plug into equation: lnk=-70700/8.314*298)=-28.54
raised to e^= 2.47e12
Hey! So the only thing I did different was using 298.15 as my temperature, which didn't make much of a difference, but I got 2.436 x 10 ^ 12. The problem is set up correctly, there might just be an error in the numbers for DeltaG.