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

Answer:

Final temperature of the gas is  576 $^{0}\textrm{C}$.

Explanation:

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

                                       $\frac{V_{1}}{T_{1}}=\frac{V_{2}}{T_{2}}$

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  $T_{2}=\frac{V_{2}T_{1}}{V_{1}}=\frac{(450mL)\times (298K)}{(158mL)}=849K$ 

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

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