A sample of 2.327 g of liquid toluene initially at 17.0 C and 0.5000 bar is rais

Question

A sample of 2.327 g of liquid toluene initially at 17.0 C and 0.5000 bar is raised to 34.0C and 3.500 bar. Use the data from Table 2.4 [Appendix] at 298.15K and I bar and assume these values are constant over the range of pressure and temperature of interest. (a) Using the density from Table 2.4, calculate the molar volume of toluene and the volume of this sample. (b) Using the approximation of Equation 3.46, calculate the change of enthalpy of the toluene sample as a result of the change of temperature and as a result of the change in pressure, and the total change of enthalpy for the process.

Explanation / Answer

a)
1 bar= 1*10^5 N/m^2
P = 0.5 bar =   0.5*10^5 = 5*10^-4 N/m^2

We have to find molar volume that is vloume of 1 mol

T = 17oC = (273+17) K = 290 K

P*V=n*R*T
(5*10^-4)* V = 1*8.314*290
V = 4.8*10^6 m^3
Answer: 4.8*10^6 m^3

b)
For solving you need to use equation 3.46.
I don't know what is that equation since you have not given that in question

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.