Question

A tank contains 111.0 g chlorine gas (Cl2), which is at a temperature of 82.0°C and absolute pressure 5.70×10⁵ Pa. The temperature of the air outside the tank is 20.0°C. The molar mass of Cl₂ is 70.9 g/mol.

(a) What is the volume of the tank?

(a) 1.50 m³
(b) 2.00 m³
(c) 2.50 m³
(d) 3.00 m³

Answer 1

The volume of the chlorine gas tank is calculated using the ideal gas law, and the result should be 7.4723 m³, which does not match any of the options provided in the question. This discrepancy indicates there may be an error in the provided choices.

Step-by-step explanation:

The volume of the tank containing chlorine gas can be calculated using the ideal gas law, which is PV = nRT. Here, P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in kelvin:

1. 
   

n = mass / molar mass = 111.0 g / 70.9 g/mol = 1.565 moles.

1. 
   

T = 82.0 °C + 273.15 = 355.15 K.

1. 
   

V = nRT / P

Plug in the values:

V = (1.565 moles) * (8.314 J/(mol·K)) * (355.15 K) / (5.70 × 10^5 Pa)

V = 7.4723 m³

None of the given options match the calculated volume, which suggests there may be an error in the question's provided choices.