Answer:
This a simple stoichiometry problem using the ideal gas law. ┬а
First take the grams of ammonium carbonate and convert it to moles using its molar mass and dividing. 11.9 g/96.0932 g/mol= .12384 mol ┬а
Now use a molar conversion using the balanced equation, ┬а
1 mol (NH4)2CO3 ---> 4 mol gas formed (2 mol NH3 + 1 mol CO2 + 1 mol H2O) = .12384 x 4 = .49535 mol gas ┬а
PV=nRT ┬а
V=nRT/P= .49535mol (.08206 Lxatm/molxK) (296K)/ (1.03 atm)=11.682 L
