Chemistry – States of matter - Solids, liquids and gases | e-Consult

We can use Charles's Law, which states that [Image missing] V₁/T₁ = V₂/T₂, where V₁ is the initial volume, T₁ is the initial temperature, V₂ is the final volume, and T₂ is the final temperature.

First, convert the temperature to Kelvin: T₁ = 27°C + 273 = 300 K. T₂ = 300 K.

We are given V₁ = 2.0 dm³, T₁ = 300 K, and P₁ = 1 atm. P₂ = 2 atm. We need to find V₂.

Charles's Law applies when pressure is constant. However, in this case, the pressure is *not* constant. We need to use Gay-Lussac's Law, which states that P₁/T₁ = P₂/T₂.

Therefore, T₂ = (P₂ * T₁) / P₁ = (2 atm * 300 K) / 1 atm = 600 K.

Now, using Charles's Law: V₂ = (V₁ * T₂) / T₁ = (2.0 dm³ * 600 K) / 300 K = 4.0 dm³.

Therefore, the new volume of the gas is 4.0 dm³.