Please show all your work, thanks in advance. 45 g of gaseous chlorine (Cl2) are

Question

Please show all your work, thanks in advance.

45 g of gaseous chlorine (Cl2) are introduced in a container (14.755 l under pressure P at temperature T. Then, the closed container is put in at thermostatic bath at a temperature 35K above T. A certain amount of Cl2 is released to bring pressure back to its initial value. After this release there are 40 g of chlorine left in the container. Calculate the initial temperature T and the initial pressure P assuming chlorine is an ideal gas. Hint: Mw Cl -35.5 g.mo

Explanation / Answer

Initial mass of Cl2 = 45 g

Volume of container = 14.755 L

Molar mass of Cl2 = 70.9 g/mol

Initial moles of Cl2 = 45 / 70.9

= 0.635

Using PV = nRT

P * 14.755 = 0.635 * 0.0821 * T

P = 0.0035 * T     .....................(1)

When temperature is is increased 35 K above T.

New mass of Cl2 = 40 g

New moles = 40 / 70.9

= 0.564

Again using PV = nRT

P * 14.755 = 0.564 * 0.0821 * (T + 35)

P = 0.00313 * (T + 35)

P = 0.00313 * T + 0.1095      .................(2)

Solving equation (1) and (2):

T = 295.94 K

Putting T in equation (1):

P = 1.03 atm

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---

---

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