Ammonium nitrite undergoes decomposition to produce only gases as shown below. nh4no2(s) → n2(g) + 2h2o(g) how many liters of gas will be produced by the decomposition of 32.0 g of nh4no2 at 525°c and 1.5 atm?

From the given balanced reaction equation:

we can see that every 1 mole of NH4NO2 will produce 1 mole of N2 and when the water also on the gas phase so, every 1 mole of NH4NO2 will produce 3 moles of gas

now we need to get number of moles of NH4NO2  = mass/molar mass
when the mass = 32 g and the molar mass of NH4NO2 = 64 mol/g

∴moles of NH4NO2 = 32 g / 64 mol/g = 0.5 mole

so, the moles that produced of gas will be = 3 * 0.5 = 1.5 moles

now, we can use the ideal gas formula to get V:

PV = nRT

when P is the pressure = 1.5 atm

n is the number of moles = 1.5 moles 

R is the ideal gas constant = 0.0821 L*atm/mol*K

and T is the temperature in Kelvin = 525 °C + 273 = 798 K

so by substitution:

1.5 atm * V = 1.5 moles * 0.0821 * 798 K

∴ V = 65.5 L

Particle exchange energy though elastic collision , hope this .