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2 years ago

A gas sample occupies 5.38L at 36.0C. what is its temperature if volume is changed to 4.86L

Chemistry

1 answer:

Alina [70]2 years ago

6 0

Answer: 2.5°C

Explanation:

Initial volume V1 = 5.38 liters

Initial temperature T1 = 36.0°C

Convert temperature in Celsius to Kelvin

(32°C + 273= 305K)

Final temperature T2 = ?

Final volume V2 = 4.68 liters

According to Charle's law, the volume of a fixed mass of a gas is directly proportional to the temperature.

Thus, Charles' Law is expressed as: V1/T1 = V2/T2

5.38/305 = 4.86/T2

To get the value of T2, cross multiply

5.38 x T2 = 4.86 x 305

5.38T2 = 1482.3

Divide both sides by 5.38

5.38T2/5.38 = 1482.3/5.38

T2 = 275.5K

Convert 275.5K to Celsius

(275.5K - 273K = 2.5°C)

Thus, the final temperature is 2.5°C

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The equilibrium constant, Kc, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C is 54.8. A reaction vessel contains 0.0890 M H

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Explanation:

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