A cylinder fitted with a piston is filled with 700 lb of saturated liquid ammonia at 15°F. The piston weighs 1 ton and has a diameter of 2.5 ft. Given Patm = 1 atm, what is the vol... A cylinder fitted with a piston is filled with 700 lb of saturated liquid ammonia at 15°F. The piston weighs 1 ton and has a diameter of 2.5 ft. Given Patm = 1 atm, what is the volume occupied by the ammonia, in ft³? Ignoring friction, determine the force required, in lbf, by mechanical attachments to hold the piston in place.

Understand the Problem
The problem describes a cylinder containing saturated liquid ammonia with a piston on top. The question asks to determine the volume of the ammonia and the force required to hold the piston in place, given the weight of the ammonia, the piston's weight and diameter, and the atmospheric pressure.
Answer
Volume of ammonia: $17.885 \, ft^3$ Force required: $0 \, lbf$
Answer for screen readers
Volume of ammonia: $17.885 , ft^3$ Force required: $0 , lbf$
Steps to Solve
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Find the specific volume of saturated liquid ammonia at 15°F
From thermodynamics tables (or software), the specific volume ($v_f$) of saturated liquid ammonia at 15°F is approximately 0.02555 $ft^3/lb$.
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Calculate the volume of the ammonia
Multiply the specific volume by the mass of the ammonia to find the total volume: $V = m \cdot v_f$ $V = 700 , lb \cdot 0.02555 , ft^3/lb = 17.885 , ft^3$
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Calculate the pressure inside the cylinder
The pressure inside the cylinder is due to the atmospheric pressure plus the pressure exerted by the piston's weight:
$P_{internal} = P_{atm} + P_{piston}$
First, calculate the area of the piston: $A = \pi r^2 = \pi (\frac{D}{2})^2 = \pi (\frac{2.5 , ft}{2})^2 = \pi (1.25 , ft)^2 \approx 4.9087 , ft^2$
Convert the piston's weight from tons to lbf (1 ton = 2000 lb): $Weight_{piston} = 1 , ton \cdot 2000 , lb/ton = 2000 , lb$
Calculate the pressure exerted by the piston: $P_{piston} = \frac{Weight_{piston}}{A} = \frac{2000 , lb}{4.9087 , ft^2} \approx 407.43 , lb/ft^2$
Convert atmospheric pressure from atm to lb/ft² (1 atm = 14.696 psi = 2116.224 lb/ft²): $P_{atm} = 1 , atm \cdot 2116.224 , lb/ft^2/atm = 2116.224 , lb/ft^2$
Now, calculate total internal pressure: $P_{internal} = P_{atm} + P_{piston} = 2116.224 , lb/ft^2 + 407.43 , lb/ft^2 = 2523.654 , lb/ft^2$
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Determine the force required to hold the piston in place
If the force is negative this means the attachments are holding piston down If the force is positive this means the attachments are holding the piston up
The force balance on the piston is: $F_{internal} = F_{atm} + F_{piston} + F_{attachments}$ $P_{internal} \cdot A = P_{atm} \cdot A + Weight_{piston} + F_{attachments}$
Therefore: $F_{attachments} = (P_{internal} - P_{atm}) \cdot A - Weight_{piston}$ $F_{attachments} = P_{piston} \cdot A - Weight_{piston}$ $F_{attachments} = 407.43 , lb/ft^2 \cdot 4.9087 , ft^2 - 2000 , lb$ $F_{attachments} = 2000 , lb - 2000 , lb = 0 , lb$
Volume of ammonia: $17.885 , ft^3$ Force required: $0 , lbf$
More Information
The force required to hold the piston in place is zero, indicating that the weight of the piston and the atmospheric pressure are perfectly balanced by the pressure of the saturated liquid ammonia.
Tips
- Forgetting to convert units (e.g., tons to pounds, psi to lb/ft²)
- Incorrectly calculating the area of the piston
- Not considering atmospheric pressure when calculating the total pressure inside the cylinder
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