# Chemistry

posted by .

The normal boiling point of bromine (Br2) is 58.8°C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol.

Calculate the value of ΔS when 1.00 mol of Br2(l) is vaporized at 58.8°C.?

• Chemistry -

dG = dH - TdS
At equilibrium (which you have at the boiling point), dG = 0, then
0 = dH -TdS
TdS = dH
dS = dH/T = ?
Remember T must be in kelvin; also dH in kJ gives dS in kJ or dH in J gives dS in J.

• Chemistry -

89.17

## Similar Questions

1. ### college chemistry-thermochemistry

i have one more question: I know this one has to do with hess's law but i'm not sure of how to get the enthalpy of vaporization from this?
2. ### chemistry

A studen is asket to calculate the amount of heat involved in changing 10.0 g of liquid bomine at room temperature (22.5 C) to vapor at 59.0 C. To do this, one must know specific heat (0.474 J/g*C), boiling point (59 C), and heat of …
3. ### Chem (Thermodynamics)

The standard molar enthalpy of fusion and the standard molar enthalpy of vaporization of benzene are 10.9 kJ/mol and 31.0 kJ/mol, respectively. Calculate the standard molar entropy changes for the solid ↔ liquid and liquid ↔ …
4. ### CHEM:

The bond enthalpy of the Br−Cl bond is equal to ƒ¢H‹ for the reaction BrCl(g) ¨ Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br−Cl bond. Br2(l)--->Br2(g) ƒ¢H=30.91 KJ/mol Br2(g)--->2Br2(g) …
5. ### chemistry:)

The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br–Cl bond. Br2(l)--->Br2(g) ÄH=30.91 KJ/mol Br2(g)--->2Br2(g) ÄH=192.9 …
6. ### chemistry:)

The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br–Cl bond. Br2(l)--->Br2(g) ÄH=30.91 KJ/mol Br2(g)--->2Br2(g) ÄH=192.9 …
7. ### Chemistry

At the normal boiling point of toluene,Δ Hvap=33.2 kJ/mol and ΔSvap= 86.5J/mol•K. What is the normal boiling point of toluene?
8. ### Chemistry

How do you calculate ΔSfus and ΔSvap for HCl given melting point,ΔHfus, boiling point, and ΔHvap also how do you determine the entropy change when 5.20 mol of HCl(l) freezes at atmospheric pressure.
9. ### Chemistry

If ammonia is manufactured at 356 K, is the reaction spontaneous, given that the enthalpy and entropy change for the reaction are -93 kJ/mol and -198 J/mol K, respectively?
10. ### chemistry

Calculate the heat of decomposition for this process at constant pressure and 25°C. (Look up the standard enthalpy of formation of the reactant and products in the table; ΔH°f(BaCO3(s)) = -1218.8 kJ/mol, ΔH°f (BaO(s)) …

More Similar Questions