Question

a balloon has a volume of 253.2 ml at 356k. the volume of the balloon is decreased to 165.4ml. determine the new temperature

Answer 1

233K

Step-by-step explanation:

V1/ T1 = V2/T2

where

V1 ( initial volume)= 253.2 mL

T1 ( initial temperature in Kelvin) = 356 K

V2( final volume)= 165.4 mL

T2( final temperature in Kelvin)= ?

Since we are trying to calculate the final temperatute, rearrange the equation to make T2 the subject and then substitute the known values.

T2= V2/(V1/T1)

T2= 165.4/(253.2/356)

T2= 232.552922591

T2= 233 K

Answer 2

Using the Ideal gas law: PV = nRT; and given the initial conditions:

V1 = 253.2 mL
T1 = 356K

We are asked to determine the new temperature if the volume of the balloon decreased to (V2 = 165.4 mL)

Assume that the pressure and number of moles are constant, the ideal gas law becomes:

V/T = constant

V1/T1 = V2/T2

Solving for T2:

253.2 ml/ 356K = 165.4 ml/T2

T2 = 232.55K