Question

How many grams of chlorine gas must be in a 10.0 L container to exert a pressure of 9.7 atm at a temperature of 25°C?

Answer 1

2.8 × 10² g

Step-by-step explanation:

Given data

• Volume (V): 10.0 L

• Pressure (P): 9.7 atm

• Temperature (T): 25°C

Step 1: Convert 25°C to the absolute scale

When working with gases, we have to convert the temperatures to the Kelvin scale, using the following expression.

K = °C + 273.15 = 25°C + 273.15 = 298 K

Step 2: Calculate the moles of chlorine gas

We will use the ideal gas equation.

`P * V = n * R * T\\n = (P * V)/(R * T) = (9.7atm * 10.0L)/((0.0821atm.L)/(mol.K) * 298K) = 4.0 mol`

Step 3: Calculate the mass of chlorine gas

The molar mass of Cl₂ is 70.91 g/mol. Then,

`4.0mol * (70.91g)/(mol) = 2.8 * 10^(2) g`