A gas sample has an original volume of 760 ml when collected at 700 mm and 40oC. If a change is made in the gas temperature which causes the volume of the gas sample to become 420 ml at 1.25 atm, what is the new temperature?

Question

Marissa Stokes

Chemistry

28 November, 20:24

A gas sample has an original volume of 760 ml when collected at 700 mm and 40oC. If a change is made in the gas temperature which causes the volume of the gas sample to become 420 ml at 1.25 atm, what is the new temperature?

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Answers (1)

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Dale Murillo · Answer 1

235k

Explanation:

To solve this problem, we will use the general gas equation.

In its simplest form, the general gas equation can be represented as follows:

P1V1/T1 = P2V2/T2

P1 = 700mmHg

V1 = 760ml

T1 = 40 degrees Celsius = 40 + 273.15 = 313.15K (conversion into standard temperature unit)

P2 = 1.25 atm

We have to covert this into the same unit as the first pressure.

760mmHg = 1atm

x mmHg = 1.25 atm

x = 1.25 * 760 = 950mmHg

V2 = 420ml

T2 = ?

Now, rearranging the equation will yield:

T2 = P2V2T1/P1V1

T2 = 950 * 420 * 313.5/700 * 760

T2 = 235.125K or - 38.025 degrees celcius