- #1
YoChem
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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 partial pressure of the gases after the reaction? (Cl2, NO, NOCl2)
What percent of NOCl decomposed?
So off the bat I'm assuming that there is 1.7 mol of NOCl, 1.7 mol NO and .85 mol of Cl2.
After that I've tried a few different things. If someone could explain the steps to me that would be great!
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 partial pressure of the gases after the reaction? (Cl2, NO, NOCl2)
What percent of NOCl decomposed?
So off the bat I'm assuming that there is 1.7 mol of NOCl, 1.7 mol NO and .85 mol of Cl2.
After that I've tried a few different things. If someone could explain the steps to me that would be great!