Here’s a table to help visualize the calculation:
| Given: | |
|---|---|
| Number of moles (n) | 0.10 mol |
| Molar volume at STP (V) | 22.4 L/mol |
|---|---|
| Calculation: | |
| Volume (V) | 0.10 mol × 22.4 L/mol |
| 2.24 liters |
Therefore, the syringe would indicate a volume of approximately 2.24 liters.
OR
We can use the molar volume of an ideal gas at STP, which is roughly 22.4 liters/mol, to calculate the volume indicated by the syringe containing 0.10 mol of neon gas at STP.
Given that there are 0.10 moles of neon gas, we can use the following equation to determine the volume:
Volume is equal to the product of the number of moles and the molar volume.
Volume is equal to 0.10 mol/22.4 L/mol.
2.24 liters in volume
As a result, the syringe would show a volume of about 2.24 liters.
or
To determine the volume of the syringe containing 0.10 mol of neon gas at STP (Standard Temperature and Pressure), we can use the ideal gas law equation:
PV = nRT
Where: P = Pressure (STP = 1 atm) V = Volume n = Number of moles R = Ideal gas constant (0.0821 L·atm/(mol·K)) T = Temperature (STP = 273.15 K)
Plugging in the values: P = 1 atm n = 0.10 mol R = 0.0821 L·atm/(mol·K) T = 273.15 K
The equation becomes: (1 atm) * V = (0.10 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)
Simplifying: V = (0.10 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K) / (1 atm)
Calculating: V ≈ 2.24 L
Therefore, the syringe would indicate a volume of approximately 2.24 liters.
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