Ammonium nitrate can decompose explosively when heated according to the equation

Question

Ammonium nitrate can decompose explosively when heated according to the equation: 2NH4NO3(s)-------2N2(g) + 4H2O(g) + O2(g) How many liters of gas would be formed at 4500C and 1.00 atm pressure by explosion of 450g of NH4NO3?

Explanation / Answer

Assume IDEAL GAS condition The reaction is 2(NH4NO3) (s) ----> 2N2 (g) + O2 (g) + 4H2O (g) PV = nRT n = mole of N2 + mole of O2 + mole of H2O, all produced in the rex mole NH4NO3 reacted = 1.57 g(1 mol/80.043g) = 0.0196 moles mole of N2 produced = 0.0196 mol (2mol N2/2mol NH4NO3) = 0.0196 mole mole of O2 produced = 0.0196 mol (1mol O2/2mol NH4NO3) = 0.00981 mole mole of H2O produced = 0.0196 mol (4mol H2O/2mol NH4NO3) =0.0392 mole Therefore, n= 0.0196 + 0.00981 + 0.0392 =0.06861 mole PV=nRT V= nRT/P T= 120 C = 393.15 K P= 737 mmHg = 0.970 atm R = 0.082?1 L?atm?K-1?mol-1 V = (0.06861 x 0.082?1 x 393.15)/ 0.970 = 2.28 L

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