Asked by Isaac Joshua
A given mass of chlorine occupies 38cm³ at 20°c. Determine its final volume at 45°c. Pressure remains constant
Answers
Answered by
GPT 3.5
In order to solve this problem, we need to assume the gas is behaving ideally. The equation that relates the initial and final volume and temperature is the following:
(V1 / T1) = (V2 / T2)
Where:
V1 = initial volume (38 cm³)
T1 = initial temperature (20°C) + 273.15 = 293.15 K (convert to Kelvin)
V2 = final volume (unknown)
T2 = final temperature (45°C) + 273.15 = 318.15 K (convert to Kelvin)
Now we can plug in the values and solve for V2:
(38 cm³ / 293.15 K) = (V2 / 318.15 K)
V2 = (38 cm³ * 318.15 K) / 293.15 K
V2 = 41.292 cm³ (rounded to three decimal places)
Therefore, the final volume of the given mass of chlorine at 45°C is approximately 41.292 cm³.
(V1 / T1) = (V2 / T2)
Where:
V1 = initial volume (38 cm³)
T1 = initial temperature (20°C) + 273.15 = 293.15 K (convert to Kelvin)
V2 = final volume (unknown)
T2 = final temperature (45°C) + 273.15 = 318.15 K (convert to Kelvin)
Now we can plug in the values and solve for V2:
(38 cm³ / 293.15 K) = (V2 / 318.15 K)
V2 = (38 cm³ * 318.15 K) / 293.15 K
V2 = 41.292 cm³ (rounded to three decimal places)
Therefore, the final volume of the given mass of chlorine at 45°C is approximately 41.292 cm³.