Answer
0.03 mol
Explanation
Given:
Volume, V = 10.88 L
Temperature, T = 10.0°C = (10.0 + 273.15 K) = 283.15 K
Pressure, P = 6.05 kPa
What to find:
The moles of neon gas in the sign.
Step-by-step solution:
The moles of neon gas in the sign can be calculated using the ideal gas equation:
[tex]\begin{gathered} PV=nRT \\ \\ \Rightarrow n=\frac{PV}{RT} \\ \\ where\text{ }n\text{ }is\text{ }the\text{ }moles \end{gathered}[/tex]R = molar gas constant = 8.314 L⋅kPa⋅K⁻¹⋅mol⁻¹
Plugging the values of the parameters into the formula, we have:
[tex]\begin{gathered} n=\frac{6.05\text{ }kPa\times10.88\text{ }L}{8.314\text{ }L⋅kPa⋅K⁻¹⋅mol⁻¹\times283.15\text{ }K}= \\ \\ n=\frac{65.824}{2354.1091\text{ }mol^{-1}} \\ \\ n=0.02796mol \\ \\ To\text{ }two\text{ }decimal\text{ }places, \\ \\ n=0.03\text{ }mol \end{gathered}[/tex]The moles of neon gas in the sign = 0.03 mol.