Consider the following reaction at 298 K:

Question

C(graphite) +2Cl2 (g) -----> CCl4(l)

Calculate the following quantities.

Delta H: -139 kJ/mol

deltaS(sys)=? J/mol*K
deltaS(surr)=? J/mol*K
deltaS(univ)=? J/mol*K

My answer is:
deltaS(sys)=654.9J/mol*K
deltaS(surr)=0.4664 J/mol*K
deltaS(univ)=655.366J/mol*K

Is this right???????????

Answer 1

Your tables may not be the same as mine but I looked and found
Cl2 for Cl2 = 223.0 J/mol
C(graphite) = 5.740
CCl4(l) = 216.4
If I use S products - S reactants that becomes 216.4 - 5.740 - (2*223.0) and I don't see anything in your answers close to that.

Answer 2

So what are the answers for
deltaS(sys)=? J/mol*K
deltaS(surr)=? J/mol*K
deltaS(univ)=? J/mol*K
I need to verify the correct answers. Could you please tell me...Thanks!

Answer 3

Also I don't know how you are working this problem out.

Answer 4

DrBob222 could you please answer!!!!!!

Answer 5

My answer is:
deltaS(sys)=654900J/mol*K
deltaS(surr)=466.4 J/mol*K
deltaS(univ)=655366J/mol*K

Sorry I forgot to convert to J

also I checked this problem and I only got thedeltaS(surr)=466.4 J/mol*K correct. Please help