Ammonium nitrate can decompose explosively when heated according to the equation:
2NH4NO3 (s) ---- > 2N2 (g) + 4H20 (g) + O2 (g)
How many liters of gas would be formed at 450° C and 1.00 atm pressure by explosion of 450 g of NH4NO3 ?
2NH4NO3 (s) ---- > 2N2 (g) + 4H20 (g) + O2 (g)
How many liters of gas would be formed at 450° C and 1.00 atm pressure by explosion of 450 g of NH4NO3 ?
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By definition, we know that one mole of any gas at STP (0 C - 273 K, and 1.0 atm of pressure) will occupy 22.4-L. So what we need to do is use stoichiometry to find the volume of gas that gets produced. Note that since all gases have a volume of 22.4 at STP, we don't have to worry that we really have 3 different gases! The balanced equation shows us 2 moles of NH4NO3 yields 7 moles of gas!
450-g NH3NO4 x 1 mole NH3NO4 x 7 moles gas x 22.4-L gas
_______________________________________ =
80-g NH4NO3 x 2 moles NH3NO4 x 1 mole gas
441-L of gas but this is at 0 C, we want its volume at 450 C!
Heating the gas volume to 450 C (723 K) will really expand this gas, volume will really be big.
Charles' law says that volume divided by Kelvin temperature is constant thus
441-L / 273 K = V2 / 723 K and V2 = 1168-L
Hope this helps...good luck with Chem!
450-g NH3NO4 x 1 mole NH3NO4 x 7 moles gas x 22.4-L gas
_______________________________________ =
80-g NH4NO3 x 2 moles NH3NO4 x 1 mole gas
441-L of gas but this is at 0 C, we want its volume at 450 C!
Heating the gas volume to 450 C (723 K) will really expand this gas, volume will really be big.
Charles' law says that volume divided by Kelvin temperature is constant thus
441-L / 273 K = V2 / 723 K and V2 = 1168-L
Hope this helps...good luck with Chem!