Question

At what pressure would a 5.32 mol Cl2 sample occupy 5.08 L at 181.59 K? please help!!

Answer 1

Answer: At a pressure of 15.613 atm a 5.32 mol $Cl_{2}$ sample occupy 5.08 L at 181.59 K.

Explanation:

Given: Moles = 5.32 mol

Volume = 5.08 L

Temperature = 181.59 K

Formula used to calculate the pressure is as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$PV = nRT\\P \times 5.08 L = 5.32 mol \times 0.0821 L atm/mol K \times 181.59 K\\P = \frac{5.32 mol \times 0.0821 L atm/mol K \times 181.59 K}{5.08 L}\\= 15.613 atm$

Thus, we can conclude that at a pressure of 15.613 atm a 5.32 mol $Cl_{2}$ sample occupy 5.08 L at 181.59 K.