2.0 L flask:
Use PV = nRT and solve for n.
1.00L flask:
Use PV = nRT and solve for n.
Add to find total mols.
Then PV = nRT and use total mols and total volume to find total pressure.
Use PV = nRT and EACH n with total volume to find partial pressure of each.
I know you don't have a temperature listed but the easy way is to make up a temperature and use that throughout. I would use the number 1 to make calculation easier; the n you get will not be the right n but that won't make any difference.
Consider the following reaction:
4NH3(g) +5O2(g) -->4NO(g) +6H2O(g)
Suppose we have two flasks connected by a stopcock. In one flask, we have 2.0L of NH3(g) at a pressure of .500 atm. In the other flask, we have 1.00L of O2(g) at a pressure of 1.5atm. When the stopcock is opened, the gases mix according to the equation above.
Calculate the partial pressure of all gases after the reaction is complete.
Calculate the total pressure after the reaction is complete. You may assume the total volume is 3.00L.
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