Achemist has a 12.5 liter sample of neon gas at 1.00 atm and 30 c. if the chemist compresses the sample to 10.5 liters and holds the pressure constant, what is the new temperature of the neon gas?

254.5 K

Explanation:

Data Given

initial volume V1 of neon gas = 12.5 L

final Volume V2 of neon gas = 10.5 L

initial Temperature T1 of neon gas = 30 °C

convert Temperature to Kelvin

T1 = °C +273

T1 = 30°C + 273 = 303 K

final Temperature T2 of neon gas = ?

Solution:

This problem will be solved by using Charles' law equation at constant pressure.

The formula used

                        V1 / T1 = V2 / T2

As we have to find out Temperature, so rearrange the above equation

                       T2 = V2 x T1 / V1

Put value from the data given

T2 = 10.5 L x 303 K / 12.5 L

T2 = 254.5K

So the final Temperature of neon gas = 254.5 K

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explanation:

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