Question

Determine the volume occupied by 10 mol of helium at 27 ° C and 82 atm

please.

Answer 1

3.00 L

Step-by-step explanation:

Convert the pressure to Pascals.

P = 82 atm × (101325 Pa/atm)

P = 8,308,650 Pa

Convert temperature to Kelvins.

T = 27°C + 273

T = 300 K

Use ideal gas law:

PV = nRT

(8,308,650 Pa) V = (10 mol) (8.314 J/mol/K) (300 K)

V = 0.00300 m³

If desired, convert to liters.

V = (0.00300 m³) (1000 L/m³)

V = 3.00 L

Answer 2

`\large \boxed{\text{3.0 L}}`

Step-by-step explanation:

`\begin{array}{rcl}pV &=& nRT\\\text{82 atm} * V & = & \text{10 mol} * \text{0.082 06 L}\cdot\text{atm}\cdot\text{K}^(-1)\text{mol}^(-1) * \text{300.15 K}\\82V & = & \text{246 L}\\V & = & \textbf{3.0 L} \\\end{array}\\\text{The volume of the balloon is $\large \boxed{\textbf{3.0 L}}$}`