If the sign contains neon at a pressure of 1.72 torr at 32 C, how many grams of neon are in the sign? (The volume of a cylinder is pie r2 h.)

You didn't post enough information to find the volume of the sign. (And note the correct spelling of pi).

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To find the number of grams of neon in the sign, we need to use the ideal gas law to calculate the number of moles of neon and then convert it to grams using the molar mass of neon.

1. Begin by writing down the given values:
- Pressure (P) = 1.72 torr
- Temperature (T) = 32°C = 32 + 273.15 = 305.15 K (converted to Kelvin)

2. Convert the pressure from torr to atmospheres (atm):
- 1 atmosphere (atm) = 760 torr
- Convert 1.72 torr to atm: 1.72 torr / 760 torr/atm = 0.00226 atm

3. Convert the volume equation to solve for the number of moles:
- Rearrange the formula for volume (V) to solve for moles (n):
V = π * r^2 * h
n = PV / (RT), where P is pressure, V is volume, R is the ideal gas constant, and T is temperature.

4. Determine the appropriate value for the ideal gas constant (R):
- R = 0.0821 L·atm/(mol·K) (in most common units)

5. Calculate the volume of the sign:
- Since we don't have the actual values for the radius (r) and height (h), we cannot directly find the volume. We need more information to proceed.

Once we have the volume of the sign, we can proceed with the remaining calculations:

6. Calculate the number of moles (n):
- n = PV / (RT)
- Substitute the given values:
n = (0.00226 atm) * (V in L) / (0.0821 L·atm/(mol·K)) * (305.15 K)

7. Convert the calculated moles to grams:
- The molar mass of neon (Ne) is approximately 20.18 g/mol.
- Multiply the number of moles by the molar mass to obtain the mass in grams.

After following these steps, you will be able to calculate the number of grams of neon in the sign once you have the volume of the sign.