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What volume of no at stp is formed from 1250 l of nh3 at 325 degrees Celsius and 4.25 ATM assuming temperature and pressure remains constant?
Wiki User
∙ 12y ago
NO → NH3
molecular proportion is 1 to 1.
Considering ideal gas behaviour as a good approximation.
Avogadro's principle states that "equal volumes of any gas at the same pressure and temperature contain the same amount of molecules".
So, 1250 L of NH3 (ammonia) at 325oC and 4.25 atm will produce the same volume of NO (nitric oxide) at the same temperature and pressure.
If such a volume of gas is needed at STP conditions (T = 25oC ≈ 298 K, P =1 atm),
we draw upon the ideal gas equation:
PV = nRT (1)
where P → pressure, V → volume, n → number of mole, R → Universal gas constant, T → Thermodynamic temperature (absolute temperature).
From (1), P1V1/T1 = n1R (2) and P2V2/T2 = n1R (3)
where 1 and 2 are the original T,P and STP conditions respectively.
From (2) and (3) → P1V1/T1 = P2V2/T2 (4)
From (4) → V2 = P 1V1T2/(P2T1) (5)
Data in (5) → V2 = 4.25 atm∙(1250 L)∙[298 K]/[(1 atm)∙(325+273) K] = 2647 L
Wiki User
∙ 12y ago
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