Recent content by YoChem

Homework Statement An empty 4 L steel vessel is filled with 1 atm of CH4 and 4 atm of O2 at 300K. A spark causes the following reaction totake place. CH4 + O2 ------> CO2 + 2H20 delta H=-802 kj What is the final temperature inside the vessel after combustion assuming that the steel...

Well I got the correct answer. If someone wanted to check my work just to make sure it wasnt blind luck. 1) I wanted to know how many moles are supposed to be in the final reaction so through the ideal gas law the final reaction should have 2.25 moles. 2) So we started with 1.7 moles of...

In your question your'e saying I have two unknown partial pressure, but don't i have 3? The NOCl as well. The sum of all the partial pressures though have to equal .26 atm. The ratio of NO/Cl2 is 1:2 correct?

Sorry maybe I am not seeing this clearly. Dont you need to know the total amount of moles to figure out the partial pressure? (mol of molecule/total mol)*(pressure)? So in this case the moles of NOCl is 1.7. The mol of NO is the same 1.7 and the mol of Cl2 is half that .85. Then I would...

So what would be the total amount of moles of gas? is it 5 (2+2+1) or 4.25 (1.7+1.7+.85) and would the pressure it gets multiplied by be .26 (the final pressure in the vessel) or is it .2 (P=((1.7)(.08206)(498)/353)). Sorry I am lost with this, my instructor kind of breezed though this...

Sorry about that. I did leave a part out. It says the final pressure after the reaction is .26 atm. Its from the Mastering Chemistry software and its for Chem 1 and we are currently studying partial pressure. We have not gone over ICE charts or anything overtly compicated. Any thoughts?

So I've been working on this for awhile now and I am just not getting to the right answer. The exact question is: When 1.7 mol of NOCl was heated to 225 C in a 353 L steel reaction vessel the NOCl partially decomposed according to the following equation: 2NOCl ---->2NO + Cl2 What are the...