A 15.37 cm diameter compressed air tank is 84.31 cm tall. The pressure at 18.25°C is 128 atm. a. How many moles of air are in the tank? b. What volume would this air occupy at STP?
Added by Zachary W.
Step 1
The tank is a cylinder, so we can use the formula for the volume of a cylinder: V = πr^2h, where r is the radius and h is the height. The diameter is 15.37 cm, so the radius is half of that: r = 15.37/2 = 7.685 cm. The height is 84.31 cm. Now we can find the Show more…
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A compressed-air cylinder stands $100 \mathrm{~cm}$ tall and has internal diameter $20.0 \mathrm{~cm} .$ At room temperature, its pressure is 180 atm. (a) How many moles of air are in the cylinder? (b) What volume would this air occupy at room temperature and 1 atm pressure?
A compressed air cylinder stands $100 \mathrm{~cm}$ tall and has internal diameter $20.0 \mathrm{~cm}$. At room temperature, the pressure is $180 \mathrm{~atm}$. (a) How many moles of air are in the cylinder? (b) What volume would this air occupy at $1.0$ atm and rooen temperature?
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