Question

425 mL of neon gas at -12°C and 788 mmHg

Answer 1

Answer:

The final temperature is 806.226 degrees celcius.

Explanation:

It is given that initial conditions are as follows,

Initial volume = $425 ml$

Initial temperature =$- 12 degrees celcius = 261 K$

Initial pressure =$788 mmHg$

The final conditions are as follows,

Final volume = $2.4 liters$

Final pressure = $577 mmHg$

Final temperature = "T"

Let R be universal gas constant, n be number of moles..

The ideal gas equation, is as follows,

$(pressure)(volume) = (number of moles)(R)(temperature)$

The number of moles remain constant in the process,

so equating initial number of moles = final number of moles , we get

$\frac{(788)(425)(10^{-3}}{261} = \frac{(577)(2.4)}{T}$

$T = 1079.226 K$ = 806.226 degrees celcius