Question

The volume of a sample gas, initially at 25 C and 158 mL, increased to 450 mL. What is the final temperature of the sample of gas, if the pressure in the container it kept constant?

Answer 1

Final temperature of the gas is 576
`^(0)\textrm{C}`.

Step-by-step explanation:

As the amount of gas and pressure of the gas remains constant therefore in accordance with Charles's law:

`(V_(1))/(T_(1))=(V_(2))/(T_(2))`

where
`V_(1)` and
`V_(2)` are volume of gas at
`T_(1)` and
`T_(2)` temperature (in kelvin scale) respectively.

Here
`V_(1)=158mL` ,
`T_(1)=(273+25)K=298K` and
`V_(2)=450mL`

So
`T_(2)=(V_(2)T_(1))/(V_(1))=((450mL)* (298K))/((158mL))=849K`

849 K = (849-273)
`^(0)\textrm{C}` = 576
`^(0)\textrm{C}`

So final temperature of the gas is 576
`^(0)\textrm{C}`.