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How do I calculate the pressure? I am completely stuck.?
A 2.1 L sample of nitrogen at 25°C and 6.5 atm is allowed to expand to 16.2 L. The temperature remains constant.
What is the final pressure?
(2 significant figures)
2 Answers
- Dr WLv 710 years agoFavorite Answer
steps to solving ALL of these 2 state gas law type problems
(1).. write down.. P1V1/(n1T1) = P2V2/(n2T2)
(2).. rearrange for your desired unknown
(3).. cancel anything held constant
(4).. solve
***********
starting with...
P1V1/(n1T1) = P2V2/(n2T2)
rearranging..
P2 = P1 x (V1/V2) x (n2/n1) x (T2/T1)
given T is constant and assuming n is constant.. which it usually is!.. T1 = T2.. n1 = n2.. so we can cancel them to get
P2 = P1 x (V1/V2)
solving
P2 = 6.5atm x (2.1L / 16.2L) = 0.84atm
*********
notice..
a).. how I grouped everything? this helps keep units consistent and the variables in the correct position
b).. how I didn't need to shout "this is boyles law" and plop down an equation.. P2 = P1 x (V1/V2) came about naturally.
*********
questions?
- Anonymous10 years ago
Boyle's law states that Volume and Pressure are directly proportional if the temperature remains constant.
You can use this formula.
Pi*Vi=Pf*Vf
Re arrange it so that
Pf=(Pi*Vi) / Vf
Plug in your numbers.
Pf=(6.5atm)(2.1L) / 16.2L
Pf = 0.84 atm.
And that's your answer!