chemistry

Doing review for an exam and I can't find how to do this problem in my notes.

2 SO2 + 2 Cl2 -----> 2 SOCl2 + O2

from a previous problem I solved:

rate=k[SO2]^2[Cl2]
k = 467.666666... or in sig. figs 467

Energy reaction:

T= 25 C
The activation energy (Ea) is 35.0kJ/mole
enthalpy of reaction (^Hrxn) is +20 kJ.

Questions:

1.) What is the activation energy of the reverse reaction?

Is this just -35 kJ/mole? If not, how do I determine?

b.) What is the value of enthalpy of reaction for the reverse reaction?

Can't find equation.


c.) What is the effect an increase in temperature would have on the rate of the reaction and on the value of the rate constant? Explain the manner in which it affects the rate and the rate constant.

Ah, a qualitative question. I believe that an increase in temp. would cause an increase in the rate of reaction b/c an increase in heat speeds up molecules. Not sure about the rate constant.

d.) Calculate the value of the rate constant for this same reaction if the temperature increased from 25 C to 35 C.

Not sure of the equation here.

e.) What is the effect the addition of a homogeneous catalyst has on the rate of a reaction and the value of a rate constant? Explain the manner in which it affects the rate and the rate constant.

I'm guessing since this is a catalyst it speeds up the reaction (by definition of a catalyst, right?). Once again, not sure about the rate constant.


Okay, I'm guessing from what I've read there is a single equation I don't have that I need.

I do have an equation kind of like what is going on here:

k=Ae^(-Ea/RT) with:
R= 8.314 J/K mol (or 8.314*10^(-3) kJ/K mol)

I'm just not sure how enthalpy of reaction is involved here, so I think I need something else.

Thank you.

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