Question

A sample of Ar gas has a pressure of 1.20 atm at 125°C and a volume of 1.00 L. What would the temperature be (°C) with a pressure of 1.80 atm and constant volume?

Answer 1

597K

Step-by-step explanation:

Given parameters:

Initial pressure = 1.2atm

Initial temperature = 125°C = 125 + 273 = 398K

Initial volume = 1.00L

Final pressure = 1.80atm

Final volume = 1.00L

Unknown:

Final temperature = ?

Solution:

To solve this problem, we must understand that at constant volume, the pressure of a given mass of gas varies directly with the absolute temperature.

Mathematically;

`(P_(1) )/(T_(1) )` =
`(P_(2) )/(T_(2) )`

where P and T are the pressures

1 and 2 are the initial and final states

Now insert the parameters and solve;

`(1.2)/(398)` =
`(1.8)/(T_(2) )`

T₂ x 1.2 = 398 x 1.8

T₂ = 597K