Question

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?

Answer 1

235k

Step-by-step 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