🤓 Based on our data, we think this question is relevant for Professor Bloxton's class at TEMPLE.
• Dinitrogen tetroxide (N2O4) – excess
• (CH3)2N2H2 – limiting reagent
Once all of the (CH3)2N2H2 is consumed, the reaction will stop because no (CH3)2N2H2 will be available to react with N2O4 anymore.
Calculate amount of each product produced from (CH3)2N2H2: mole to mole comparison
Some very effective rocket fuels are composed of lightweight liquids. The fuel composed of dimethylhydrazine [(CH3)2N2H2] mixed with dinitrogen tetroxide was used to power the Lunar Lander in its missions to the moon. The two components react according to the following equation:
(CH3)2N2H2(l) + 2N2O4(l) → 3N2(g) + 4H2O(g) + 2CO2(g)
If 150 g dimethylhydrazine reacts with excess dinitrogen tetroxide and the product gases are collected at 127°C in an evacuated 250-L tank, what is the partial pressure of nitrogen gas produced and what is the total pressure in the tank assuming the reaction has 100% yield?
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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.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Bloxton's class at TEMPLE.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.