Answer:
Gas must be cooled to -22.4°C
Explanation:
As volume and the moles for this gas keeps on constant, the temperature changes according to the pressure, in a directly proportion.
Pressure decrease → T° decrease
Pressure increase → T° increase
We convert the T° to Absolute value → T°C + 273
17°C + 273 = 290 K
P₁ / T₁ = P₂ / T₂ → 250 mmHg / 290K = 216 mmHg / T₂
T₂ = 216 mmHg . 290K / 250mmHg → 250.5 K
We convert the Absolute T° to °C → 250.5 K - 273 = -22.4 °C
Answer:
The gas must be cooled to a temperature of 250.6 K (or -22.6 °C)
Explanation:
Step 1: Data given
Initial pressure = 250 mm Hg =
Initial temperature = 17.0 °C = 290 K
Final pressure = 216 mm Hg
Step 2: Calculate new temperature
P1/T1 = P2/T2
⇒ with P1 = the initial pressure = 250 mm Hg =
⇒ with T1 = the initial temperature = 290 K
⇒ with P2 = the new pressure = 216 mm Hg =
⇒ with T2 = the new temperature = TO BE DETERMINED
250/ 290 = 216/ T2
0.862 = 0.216/T2
T2 = 0.216/0.862
T2 = 250.6 K = -22.6°C
The gas must be cooled to a temperature of 250.6 K (or -22.6 °C)
