Chem! 15 pts + brainliest

Using Ideal Gas law, what is the volume of 5.00 mol of helium at 393.15 degrees Kelvin and 1520 mmHg?

Question 17 options:

1206 L

80.7 L

10.96 L

V = 80.65L

Explanation:

Volume = ?

Number of moles n = 5 mol

Temperature (T) = 393.15K

Pressure = 1520mmHg

Ideal gas constant (R) = 62.363mmHg. L/mol. K

According to ideal gas law,

PV = nRT

P = pressure of the ideal gas

V = volume the gas occupies

n = number of moles of the gas

R = ideal gas constant (note this can varies depending on the unit of your variables)

T = temperature of the ideal gas

PV = nRT

Solve for V,

V = nRT / P

V = (5 * 62.363 * 393.15) / 1520

V = 80.65L

The volume the gas occupies is 80.65L