Friday

October 31, 2014

October 31, 2014

Posted by **Desiree** on Monday, March 19, 2012 at 10:22pm.

A gas occupies 340mL at 273 K and 610 torr. What final temperature would be required to increase the pressure to 1 atm, the volume being held constant?

P1/T1 = P2/T2

T2 = (T1*P2)/ P1

1 atm = 760 torr

So,

T2 = (273 K * 760 torr)/610 torr

T2 = 340 K

- Chemistry -
**DrBob222**, Monday, March 19, 2012 at 10:26pm340 K is correct.

**Answer this Question**

**Related Questions**

Chemistry - Please help me get started, i'm not asking for the answer, just some...

chemistry - I am now stumped on another problem. How many times greater is the ...

Chemistry - Determine the molar mass of each of the following gases? A. 2.90 g ...

Chemistry - A mole of gas at 0 degrees C and 760 mmHg occupies 22.41 L. What is ...

chemistry - i keep trying to do these problems and i don't understand them. ...

chemistry - Determine the density of methane (CH4) in g/L at 24.7oC and 1.1 atm...

chemistry - I'm having a problem with the gas constant. This is it: In the ...

Chemistry - If the equilibrium concentrations are [PCl5] = 1.0M, [Cl2] = 0.10M, ...

calculus - please help with this problem- i've been working for the last 2 hours...

algebra II - I have been working on this problem for a while and for some reason...