Question

A compressed air cylinder stands 100 cm tall and has internal diameter 20.0 cm. At room temperature, the pressure is 180 atm. (a) How many moles of air are in the cylinder? (b) What volume would this air occupy at 1.0 atm and room Temperature

Answer 1

We have that The  moles of air are in the cylinder and the volume would this air occupy at 1.0 atm and room Temperature is

• V=5651.997L
• n=229.756

From the question we are told

• A compressed air cylinder stands 100 cm tall
• internal diameter 20.0 cm
• At room temperature, the pressure is 180 atm

Generally the equation for the Volume of Cylinder  is mathematically given as

$V=\pi r^2l\\\\V=\pi *{\frac{20}{2*100}}*1\\\\V=31.4L$

Therefore

The equation for the ideal gas  is mathematically given as

$PV=nRT\\\\n=\frac{PV}{RT}\\\\n=\frac{180*31.4}{0.082*300}\\\\n=229.756$

Generally the equation for the ideal gas  is mathematically given as

$PV=nRTWhere\\\\V=\frac{nRT}{P}\\\\V=229.756*0.082*300\\\\V=5651.997L$

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