Question

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

expands into a 2.40 L container while the
pressure decreases to 577 mmHg. What is the
temperature of the gas in °C?
Enter the answer

Answer 1

The final temperature is 806.226 degrees celcius.

Step-by-step 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

`((788)(425)(10^(-3))/(261) = ((577)(2.4))/(T)`

`T = 1079.226 K` = 806.226 degrees celcius