[Corribus]

8.31446 J/mol K.  You can convert to kJ/mol K, but it's not 0.0831446; try 0.00831446.   Looks like you need to start being a lot more careful with the basics.  This is why you are not getting correct answers.

[webassignbuddy]

8.31446 J/mol K.  You can convert to kJ/mol K, but it's not 0.0831446; try 0.00831446.   Looks like you need to start being a lot more careful with the basics.  This is why you are not getting correct answers.

Ok thank you!
I'm gonna try it out

[Corribus]

LOL, and then I go and I type it into LA Tex wrong.  Try this one.

[tex]\ln \frac{k_2}{k_1}=\frac{-\Delta H^o}{RT} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)[/tex]

(I put the k2 and k1 in the wrong order earlier...)

[magician4]

(...)
^ That doesn't make any sense

your right here: numbers without dimensions are meaningless (and you better should have put in dimensions in your calculatons right from the start), esp. if you miscalculate additionally

... and by doing better, my results next to perfectly match with @Corribus' results


regards

Ingo

[webassignbuddy]

LOL, and then I go and I type it into LA Tex wrong.  Try this one.

[tex]\ln \frac{k_2}{k_1}=\frac{-\Delta H^o}{RT} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)[/tex]

(I put the k2 and k1 in the wrong order earlier...)

Wait but, I know T₂ and T₁, But what does T equal in ΔH's denominator?

[Corribus]

/facepalm

[tex]\ln \frac{k_2}{k_1}=\frac{-\Delta H^o}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)[/tex]

That's what I get for scolding you about being careful...

[webassignbuddy]

/facepalm

[tex]\ln \frac{k_2}{k_1}=\frac{-\Delta H^o}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)[/tex]

That's what I get for scolding you about being careful...

Ohh...haha thank you!

[webassignbuddy]

/facepalm

[tex]\ln \frac{k_2}{k_1}=\frac{-\Delta H^o}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)[/tex]

That's what I get for scolding you about being careful...

Ok so I'm stumped again.
I got ΔH fine (54.7 kJ/mol) but for some reason I'm getting ΔS = 2.41.

I did.

ΔG_{298.15 K} = ΔH - TΔS
774.95 = 54.7 - (298.15)ΔS
774.95 - 54.7 =  -(298.15)ΔS
720.25 =  -(298.15)ΔS
720.25/(-298.15) = ΔS
-2.4157 = ΔS

[magician4]

man, use DIMENSIONS!

and RECALCULATE ΔG_298,15K : you miscalculated there!


regards

Ingo

[webassignbuddy]

man, use DIMENSIONS!

and RECALCULATE ΔG_298,15K : you miscalculated there!


regards

Ingo

ok...

ΔG_{298.15 K} = -RTln K
ΔG_{298.15 K} = -(0.008314 kJ/mol K)(298.15 K)ln (1.00 x 10^-14)
ΔG_{298.15 K} = -(0.008314 kJ/mol K)(298.15 K)(-32.236)
ΔG_{298.15 K} = (-2.478 kJ/mol)(-32.236)
ΔG_{298.15 K} = 79.9?

[magician4]

ΔG_{298.15 K} = 79.9?

79.9 of WHAT ? EGGS? years of unconciousness?

USE DIMENSIONS ... else you NEVER get the difference ΔG(T) - ΔH right, and hence NEVER will find a meaningfull solution for ΔS

[webassignbuddy]

ΔG_{298.15 K} = 79.9?

79.9 of WHAT ? EGGS? years of unconciousness?

USE DIMENSIONS ... else you NEVER get the difference ΔG(T) - ΔH right, and hence NEVER will find a meaningfull solution for ΔS

79.9 kJ/mol

And I got the right answer for ΔS and I ALSO included dimensions!

[magician4]

congratulations!


regards

Ingo

[Corribus]

LOL, well done. How many more problems in your problem set now?

[webassignbuddy]

LOL, well done. How many more problems in your problem set now?

2 more!

And thanks again to both of you for ALL of the help though and the clarification!

This next one is kind of throwing me off also...