Ammonium nitrate can decompose explosively when heated according to the equation

Question

Ammonium nitrate can decompose explosively when heated according to the equation 2 NH_4NO_3(s) rightarrow 2 N_2(g) + 4 H_2O(g) + O_2(g) How many liters of gas would be formed at 450 degree C and 1.00 atm pressure by explosion of 450 g of NH_4NO_3? At 46 degree C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth (0.10) of the original value at the same temperature? A 36.4-L volume of methane gas is heated from 25 degree C to 88 degree C at constant pressure. What is the final volume of the gas? A compound of P and F was analysed as follows: Heating 0.2324 g of the compound in a 378-cm^3 container turned all of it to gas, which had a pressure of 97 3 mmHg at 77 degree C. Then the gas was mixed with calcium chloride solution, which turned all of the F to 0.2631 g of CaF_2. Determine the molecular formula of the compound.

Explanation / Answer

Data.

T = 450° C + 273 = 723 K

P = 1 atm

mass NH4NO3 = 450 g ; m.wt = 80.043 g/mol

We have to use ideal gas law and find n for gas. But for this we have to find first the moles of reactant:

Balanced Equation:

2 NH4NO3 (s) ---> 2 N2 (g) + 4 H2O (g) + O2 (g)

2 moles NH4NO3 : 7 moles of gas

moles NH4NO3 = 450g / (80.043 g/mol)

= 5.6219 moles NH4NO3

moles of gas = n = 7 moles of gas / (2 x moles NH4NO3) = 7/2 x 5.6219

= 19.6766 moles of gas

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From Ideal gas law:

PV = nRT

V = nRT/P

V = (19.6766 moles of gas) x (0.082 atm.L/mol.K) x (723 K) / (1 atm)

V = 1166.54 L = 1.17 x 103 L

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