chemistry

posted by .

Consider the following reaction at 298 K:
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)=-253.3J/mol*K
deltaS(surr)=466.4 J/mol*K
deltaS(univ)=231.4 J/mol*K

Delta (surr) and (univ) are correct. But delta (sys) is wrong...please help thanks!

  • chemistry -

    How did you calculate the dS sys? What values did you use?

  • chemistry -

    Change in Hf(kJ/mol) Change in G Change in S

    C(graphite) 0 0 5.7
    Cl2 0 0 223.1
    CCl4 -139 -68.6 214.4

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem

    I don't believe I'm getting the correct answers for this problem. Could someone look over my work and verify whether it is correct or not?
  2. chemistry

    Given the following data at 298K, calculate delta S for : 2Ag2O(s) -> 4Ag(s) +O2(g) deltaS(J/mol.K)121.3 42.6 205.2
  3. chemistry

    Given the following data at 298K, calculate delta S for : 2Ag2O(s) -> 4Ag(s) +O2(g) deltaS(J/mol.K)121.3 42.6 205.2
  4. chemistry

    Consider the following reaction at 298 K: C(graphite) +2Cl2 (g) -----> CCl4(l) Calculate the following quantities. Delta H: -139 kJ/mol deltaS(sys)=?
  5. DrBob222

    I know I posted this but you didn't answer! Please help!!!! Consider the following reaction at 298 K: C(graphite) +2Cl2 (g) -----> CCl4(l) Calculate the following quantities. Delta H: -139 kJ/mol deltaS(sys)=?
  6. DrBob222 PLEASE HELP!

    I posted this question already but you never replied back :( Consider the following reaction at 298 K: C(graphite) +2Cl2 (g) -----> CCl4(l) Calculate the following quantities. Delta H: -139 kJ/mol deltaS(sys)=?
  7. college chem 2

    Calculate the deltaS univ for the dissolving of NaCl at room temp. S' NaCl(s)=72.11 J/k*mol; S' NaCl(aq)=115.5 J/k*mol;deltaH' NaCl(s)=-411.12 kJ/mol; deltaH' NaCl(aq)=-407.27 kJ/mol.
  8. AP Chemistry

    Calculate the entropy change when 4.88 g of H2 reacts with O2 according to the reaction 2H2(g) + O2(g)→2H2O(ℓ)at 298 K and 1 atm pressure. The standard molar enthalpy of formation of H2O(ℓ)at 298 K is −285.8 …
  9. chemistry

    In which case will the equilibrium constant (K) be less than 1 at 298 K?
  10. Chemistry

    Determine the entropy change when 1.80 mol of HBr(g) condenses at atmospheric pressure?

More Similar Questions