Solution Found!
Chlorine is produced from sodium chloride by thé
Chapter 6, Problem 71P(choose chapter or problem)
Chlorine is produced from sodium chloride by the electrochemical chlor-alkali process. During the process, the chlorine is collected in a container that is isolated from the other products to prevent unwanted (and explosive) reactions. If a \(15.50-L\) container holds \(0.5950 kg\) of \(\mathrm{Cl}_{2}\) gas at \(225^{\circ} \mathrm{C}\), calculate
(a) \(P_{\text {IGL }}\)
(b) \(P_{\text {VDW }}\left(\text { use } R=0.08206 \frac{\mathrm{atm} \cdot \mathrm{L}}{\mathrm{mol} \cdot \mathrm{K}}\right)\)
Equation Transcription:
Cl2
225°C
Text Transcription:
15.50-L
0.5950 kg
Cl_2
225°C
P_IGL
P_VDW (use R=0.08206 atm times L/mol times K)
Questions & Answers
QUESTION:
Chlorine is produced from sodium chloride by the electrochemical chlor-alkali process. During the process, the chlorine is collected in a container that is isolated from the other products to prevent unwanted (and explosive) reactions. If a \(15.50-L\) container holds \(0.5950 kg\) of \(\mathrm{Cl}_{2}\) gas at \(225^{\circ} \mathrm{C}\), calculate
(a) \(P_{\text {IGL }}\)
(b) \(P_{\text {VDW }}\left(\text { use } R=0.08206 \frac{\mathrm{atm} \cdot \mathrm{L}}{\mathrm{mol} \cdot \mathrm{K}}\right)\)
Equation Transcription:
Cl2
225°C
Text Transcription:
15.50-L
0.5950 kg
Cl_2
225°C
P_IGL
P_VDW (use R=0.08206 atm times L/mol times K)
ANSWER:
Solution 71P
Here, We have to calculate the pressure of chlorine gas by using ideal gas equation and vander waal’s expression.
Step 1 of 3
Let’s calculate the number of mole of Cl2
Number of moles of Cl2 =
Given weight of chlorine = 0.5950 kg
Convert the Kg into grams.
1 Kg = 1000gm
So, the conversion factor is
0.5950 kg
= 595 gm.
Moles of Cl2 = = 8.39 mol
Therefore, moles of chlorine gas is 8.39 mol.
______________________________________________________________________________