If i initially have a gas with a pressure of 84kPa and a temperature of 35 Celsius and I heat it up to 230 degrees Celsius, what will the new pressure be?  Assume that the volume of the container is constant.  

Expert Answers

An illustration of the letter 'A' in a speech bubbles

For this problem, we can use the gas relationship between pressure and temperature at constant volume. This gas law is also called as the Gay-Lussac’s Law which states that:

P is directly proportional to T; as the pressure of the container increased, the total temperature will increase.

``P = k...

Unlock
This Answer Now

Start your 48-hour free trial to unlock this answer and thousands more. Enjoy eNotes ad-free and cancel anytime.

Start your 48-Hour Free Trial

For this problem, we can use the gas relationship between pressure and temperature at constant volume. This gas law is also called as the Gay-Lussac’s Law which states that:

P is directly proportional to T; as the pressure of the container increased, the total temperature will increase.

``P = k T` `

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

Now, for comparing the same substance at two different conditions, this can be expressed as:

``(P_1)/(T_1) = (P_2)/(T_2)` `

OR

``(P_1)(T_2) = (P_2)(T_1)` `

From this we can solve the problem.

Given:

P1 = 84 kPa  -> initial pressure

T1 = 35 + 273.15 = 308.15K -> initial temperature

T2 = 230 + 273.15 = 503.15 K -> final temperature

P2 = x (unknown) -> final pressure

Substitute the given values and solve for the unknown:

``(P_1)(T_2) = (P_2)(T_1)` `

`(84)(503.15) = (x)(308.15)`

`X = (84*503.15)/(308.15)`

X = 137 kPa = Pressure at 230 degrees Celsius

 

 

Approved by eNotes Editorial Team