When the volume of a gas is changed from 1145 ml to 765 ml, the temperature will change from? k to 640 k?

The answer is: T1 = 957.91K

Explanation:

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The data we have are:

V1: 1145ml

V2: 765ml

T2: 640K

From the equation of the ideal gas, we have that the pressure is the same, the constant of the gases R is the same and the number of moles is the same.

We match the equations and we have:

V1 / T1 = V2 / T2

We have to find out T1:

T1 = (V1 * T2) / V2

T1 = (1145ml * 640K) / 765ml

T1 = 957.91K

The answer is: T1 = 957.91K

The according to the combined gas equation, the ratio of the initial volume to the initial volume should be equal to the ratio of the test volume to the test temperature, I. e, V1/T1=V2/T2

1145ml/T1=765ml/640K

T1 = (1145ml*640K) 765ml

=957.91K