To determine the resulting volume of chlorine gas when the temperature is adjusted from 20°C to 318 K while keeping the pressure constant, we can use the ideal gas law. The ideal gas law states that:
PV = nRT
Where: P = Pressure V = Volume n = Number of moles of gas R = Ideal gas constant T = Temperature
Since the pressure is constant, we can rearrange the equation as follows:
(V1/T1) = (V2/T2)
Where: V1 = Initial volume T1 = Initial temperature V2 = Final volume (to be determined) T2 = Final temperature
Given: V1 = 15 dm³ T1 = 20°C = 20 + 273.15 = 293.15 K T2 = 318 K (provided temperature adjustment) P = Constant (not given explicitly)
Substituting the given values into the equation:
(15 dm³ / 293.15 K) = (V2 / 318 K)
To find V2, we can solve for it:
V2 = (15 dm³ / 293.15 K) * 318 K V2 ≈ 16.214 dm³
Therefore, when the temperature is adjusted to 318 K while maintaining the same pressure, the resulting volume of the chlorine gas is approximately 16.214 dm³.