Question

A sample of gas in a balloon has a temperature of (+ 23.1oC), a current volume of 15.93 L and a pressure of 763 mmHg. If the balloon rises in the atmosphere and takes on a new volume of 45 .00 L at a pressure of 720 mmHg, what is the temperature at this altitude?

Answer 1

516°C is the temperature at this altitude.

Step-by-step explanation:

The combined gas equation is,

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

where,

`P_1` = initial pressure of gas in balloon = 763 mmHg

`P_2` = final pressure of gas in balloon= 720 mmHg

`V_1` = initial volume of gas in balloon= 15.93 L

`V_2` = final volume of gas in balloon= 45.00L

`T_1` = initial temperature of gas in balloon=
`23.1^oC=273+23.1=296.1 K`

`T_2` = final temperature of gas in balloon= ?

Now put all the given values in the above equation, we get:

`(763 mmHg* 15.93 L)/(296.1 K)=(720 mmHg* 45.00L)/(T_2)`

`T_2=789 K=789-273 ^oC=516^oC`

516°C is the temperature at this altitude.