We are given the initial partial pressures and volumes 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 :
Now before we calculate, make sure that the units are the same as the units of the gas constant R. If not, we convert. Assume room temperature.
Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide:
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
Assume this reaction is carried out in the apparatus diagramed below.
The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume 100% yield for the reaction, assume the final container volume is 3.00 L, and assume the temperature is constant.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
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Based on our data, we think this problem is relevant for Professor Demoin's class at UARK.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.