# Problem: 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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###### FREE Expert Solution

• 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 ###### Problem Details

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?