January 11, 2025, 05:14:49 PM
Forum Rules: Read This Before Posting


Topic: Boyle's Law  (Read 3828 times)

0 Members and 1 Guest are viewing this topic.

Offline ghostanime2001

  • Regular Member
  • ***
  • Posts: 65
  • Mole Snacks: +0/-8
Boyle's Law
« on: August 15, 2010, 01:37:13 AM »
1. The problem statement, all variables and given/known data
Atmospheric pressure is 100 kPa and a depth of 1m in water is equivalent in pressure to 10 kPa. A jam tin, open end down, is forced under water until the water half fills the can. At this stage, how far beneath the surface is the can? (ans is 10 m)


2. Relevant equations
I DONT'T UNDERSTAND WHY 10 metres! T_T


3. The attempt at a solution
So from what I know, I must use Boyle's Law.
P1 = 100 kpa
P2 = ?
V1= ?
V2 = 1/2 V1

P1V1=P2V2
100V1=P2(1/2 V1)
100V1=1/2 P2V1 <---Don't the V1's cancel out?
200=P2

using ratio's:
1m/10 kPa = x/200 kPa
x=20 m

Why is my answer different from my worksheet (10m) ??

Any help is greatly appreciated!
Thanks

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27895
  • Mole Snacks: +1816/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Boyle's Law
« Reply #1 on: August 15, 2010, 04:05:09 AM »
200=P2

Correct.

Where does this pressure comes from?
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline ghostanime2001

  • Regular Member
  • ***
  • Posts: 65
  • Mole Snacks: +0/-8
Re: Boyle's Law
« Reply #2 on: August 15, 2010, 05:55:13 PM »
water PLUS atmospheric pressure ?

Offline ghostanime2001

  • Regular Member
  • ***
  • Posts: 65
  • Mole Snacks: +0/-8
Re: Boyle's Law
« Reply #3 on: August 15, 2010, 10:30:33 PM »
What?

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27895
  • Mole Snacks: +1816/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Boyle's Law
« Reply #4 on: August 16, 2010, 02:02:35 AM »
water PLUS atmospheric pressure ?

Yes. How much of those 200 kPa is water?
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline ghostanime2001

  • Regular Member
  • ***
  • Posts: 65
  • Mole Snacks: +0/-8
Re: Boyle's Law
« Reply #5 on: August 16, 2010, 07:29:28 PM »
100 Kpa? 100 Kpa from atmosphere already

Sponsored Links