Question

The pressure inside a hydrogen-filled container was 2.48 atm at 21 oC. What would the pressure be if the container was heated to 84 oC ?

Answer 1

3.01 atm

Step-by-step explanation:

According to Gay-Lussac's law, the pressure (P) of a given mass of gas when volume is left constant is directly proportional to the kelvin temperature (T) of the gas. i.e

P ∝ T

P = kT

Where;

k = proportionality constant

=>
`(P)/(T)` = k

=>
`(P_(1) )/(T_(1) )` =
`(P_(2) )/(T_(2) )` -------------------(i)

Where;

`P_(1)` and
`P_(2)` are the initial and final pressures of the gas

`T_(1)` and
`T_(2)` are the initial and final temperatures of the gas

From the question;

`P_(1)` = 2.48 atm

`P_(2)` = ?

`T_(1)` = 21°C = (21 + 273)K = 294K

`T_(2)` = 84°C = (84 + 273)K = 357K

Substitute these values into equation (i) as follows;

=>
`(2.48)/(294)` =
`(P_(2) )/(357)`

Solve for
`P_(2)`

`P_(2)` =
`(2.48 X 357)/(294)`

`P_(2)` = 3.01 atm

Therefore the pressure will be 3.01 atm