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Answer:
43.1atm is the pressure using gas law and 27.2atm using Van der Waals Law.
Explanation:
Ideal gas law is:
PV = nRT
<em>Where P is pressure in atm</em>
<em>V is volume = 4.00L</em>
<em>n are moles of the gas (For chlorine Molar Mass: 70.90g/mol):</em>
<em>500g * (1mol / 70.90g) = 7.052 moles</em>
<em>R is gas constant = 0.082atmL/molK</em>
<em>T is absolute temperature = 25°C + 273 = 298K</em>
To solve the pressure, P:
P = nRT/V
P = 7.052mol*0.082atmL/molK*298K / 4.00L
P = 43.1atm is the pressure using gas law.
Van der Waals equation is:
<em>Where a is 6.58L²atm*mol⁻²</em>
<em>b = 0.056Lmol⁻²</em>
Solving for pressure:
P = 172.323 / 3.6051 - 20.4866
P = 27.2atm using Van der Waals Law