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Problem: A 20.0-L stainless steel container at 25°C was charged with 2.00 atm of hydrogen gas and 3.00 atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at 25°C? If the exact same experiment were performed, but the temperature was 125°C instead of 25°C, what would be the pressure in the tank?

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FREE Expert Solution

First, we have to write the reaction of oxygen gas and hydrogen gas to form water vapor (gas):


Next, since we are given only the initial partial pressures of the reactants, we have to use the ideal gas law to calculate the moles of each. The ideal gas law can be manipulated to isolate the moles :

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Problem Details

A 20.0-L stainless steel container at 25°C was charged with 2.00 atm of hydrogen gas and 3.00 atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at 25°C? If the exact same experiment were performed, but the temperature was 125°C instead of 25°C, what would be the pressure in the tank?