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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