Question

Determine the volume of 5,0 moles of gases (ideal gas) at STP. STP = Standard Temperature and Pressure. Standard temperature (t) = 0 oC Standard pressure (P) = 1 atm =1.013 x 105 PaUniversal gas constant (R) = 8.315 Joule/mole.Kelvin​

Answer 1

Answer:

0.112 m³

Explanation:

Use Boyle's law

$PV=\nu RT$

Determine volume from this law

$V=\frac{\nu RT}{P}=\frac{5*8.315*273}{1.013*10^5}=0.112 m^3$

Answer 2

To determine the volume of 5.0 moles of an ideal gas at STP (Standard Temperature and Pressure), you can use the ideal gas law equation:

PV = nRT

Where: P = Pressure (in Pa) V = Volume (in m³) n = Number of moles R = Universal gas constant (8.315 J/mol·K) T = Temperature (in Kelvin)

Given that: Standard temperature (t) = 0 °C = 273.15 K (convert to Kelvin) Standard pressure (P) = 1 atm = 1.013 x 10^5 Pa Number of moles (n) = 5.0 moles Universal gas constant (R) = 8.315 J/mol·K

Plug in the values and solve for V:

V = (nRT) / P V = (5.0 mol * 8.315 J/mol·K * 273.15 K) / 1.013 x 10^5 Pa V ≈ 1.23 m³

Therefore, the volume of 5.0 moles of the ideal gas at STP is approximately 1.23 cubic meters.