A gas is confined in a rigin container and exerts a pressure of 250 mm of hg at a temp at 17c. TO what temp must gas be cooled in order its pressure to become 216 mm Of hg?

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

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)

h let me think

the correct option is c.

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