The pressure inside a hydrogen-filled container was 2.12 atm at 21 degrees C. What would the pressure be if the container was heated to 79 degrees C ?

asked by @robertg24 • 11 months ago • Chemistry • 5 pts
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2 answers

We have an initial pressure of P1= 2.12 atm, and an initial temperature of T1= 21C, an unknown final pressure P2= x, and a final temperature of T2= 79C.

All of these fit perfectly into the Gay Lussac's Law formula of (P1)(T1)=(P2)(T2)

The temperatures have to be in Kelvin so remember to add 273 to your temperatures to make them from C to K.

All we have to do to isolate P2 is divide the (P1)(T1) by (T2) giving us the formula: (P1)(T1)/(T2)=(P2)

Your units of K cancel out and you're left with a pressure in atm.

Good Luck!

answered by @tylerh61 • 11 months ago

Hi @tylerh61! You were right to use the Gay-Lussac's law but the actual equation for it is P1/T1=P2/T2 instead of (P1)(T1)=(P2)(T2)

So P2=(P1*T2)/T1

Calculating it we get

P2=(2.12atm*(79+273)K)/(21+273)K

P2= 2.53823 atm

answered by @reyn • 11 months ago
  • Haha that's right, its been a bit since general chem 1 for me! Tyler commented 11 months ago
  • It's totally fine! :) Reyn commented 11 months ago