Ammonium carbonate decomposes upon heating according to the balanced equation: (

Question

Ammonium carbonate decomposes upon heating according to the balanced equation: (NH4)2 CO3(s) -> 2NH3(g) +CO2(g) + H2O(g) Calculate the total volume of gas produced at 22 Celcius and 1.07atm by the complete decomposition of 11.89g of ammonium carbonate. V= total T= 22C P= 1.07atm 11.89g(NH4)2 CO3*(1mol/120.13g)*(2mol/1mol) = 0.19795 VNH3 = nRT/P = 4.4806NH3 VCO2 = 2.2403 VH2O = 2.2403 Vtotal = 8.96 but when I submit my answer it said is wrong please help

Explanation / Answer

This a simple stoichiometry problem using the ideal gas law. 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 Now use a molar conversion using the balanced equation, 1 mol (NH4)2CO3 ---> 4 mol gas formed (2 mol NH3 + 1 mol CO2 + 1 mol H2O) = .12384 x 4 = .49535 mol gas PV=nRT V=nRT/P= .49535mol (.08206 Lxatm/molxK) (296K)/ (1.03 atm)=11.682 L

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