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To study a key fuel-cell reaction, a chemical engineer has
Chapter 6, Problem 93P(choose chapter or problem)
To study a key fuel-cell reaction, a chemical engineer has 20.0-L tanks of H2 and of O2 and wants to use up both tanks to form 28.0 mol of water at 23.8°C. (a) Use the ideal gas law to find the pressure needed in each tank, (b) Use the van der Waals equation to find the pressure needed in each tank. (c) Compare the results from the two equations.
Questions & Answers
QUESTION: Problem 93P
To study a key fuel-cell reaction, a chemical engineer has 20.0-L tanks of H2 and of O2 and wants to use up both tanks to form 28.0 mol of water at 23.8°C. (a) Use the ideal gas law to find the pressure needed in each tank, (b) Use the van der Waals equation to find the pressure needed in each tank. (c) Compare the results from the two equations.
ANSWER:
Solution 93P:
Step 1:(a)
Here, we have to calculate the pressure of each gas required in the tank.
The balanced equation for the formation of water is
Given that,
Mole of water = 28.0 mol
From the equation,
The mole of H2(g) = 28.0 mol =28.0 mol
Similarly,
The mole of O2(g) = 28.0 mol =14.0 mol