A 90.0 L stainless steel container was charged with 4.00 atm of hydrogen gas and 5.00 atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at a constant temperature of 25°C?
b. What is the pressure in the tank at a constant temperature of 125°C?
2007-10-16 17:17:39 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Do you get what I try to teach you here?
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A few more words:
the reaction is: 2H2(gas) + O2(gas) ===> 2H2O(gas)
The first important concept is: the volume of liquid water formed is negligible compared to its volume in the gas phase. Hence at 25°C, water is in the liquid phase, and its vapor pressure is small enough compared to 4.00atm, thus can also be neglected.
So at 25°C, you are "taking" every 2 portions of H2 and one portion of O2 away.
At 125°C, you are "taking" every 2 portions of H2 and one portion of O2 away, and "putting" back 2 portions H2O back.
2007-10-18 06:03:16 · answer #1 · answered by Hahaha 7 · 0⤊ 0⤋