Posted by Sarah on Wednesday, November 14, 2012 at 6:21pm.
mols NH4NO2 (is that what you meant to type?) = grams/molar mass = about 5 mols but you need to confirm that.
Therefore, you must have produced 5 mols N2 and 10 mols H2O for a total of 15 mol.
Use PV = nRT and solve for V in L.
Related Questions
Chemistry - Container A holds 752 mL of ideal gas at 2.40 atm. Container B holds...
Chemsitry II - The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is ...
Chemsitry II - mole fraction is equal to partial pressure divided by the total ...
Chemistry 101 - Are these correct? 1. A sample of gases contains three gases at ...
chemistry - The gases in a mixture have the following partial pressures at the ...
chemistry - Suppose two gases in a container have a total pressure of 1.20 atm. ...
chem - A 2.5L flask @ 15 degrees C cntains three gases. The partial pressure of ...
chemistry - a mixture of 3 gases a, b and c is at a total pressure of 6.11 atm ...
Chemistry - A 7.30-L container holds a mixture of two gases at 45 °C. The ...
chemistry - A sample of gas with a volume of 2.0 L exerts a pressure of 1.0 atm...
For Further Reading
