Reaction of gases/ gas stoichiometry

AI Thread Summary
The discussion focuses on gas stoichiometry and the application of Avogadro's Law in determining the volume of products formed from gas reactions. For the reaction of 50 mL of H2 and 50 mL of N2, the stoichiometric ratio indicates that 50 mL of ammonia (NH3) will be produced. In a separate example involving 50 mL of chlorine gas and 50 mL of ethylene, the product volume is also 50 mL due to the conservation of moles in the reaction. Participants clarify that volumes can be treated as moles under constant temperature and pressure, emphasizing the importance of understanding limiting reagents in gas reactions. The overall conclusion reinforces that the total volume of gaseous products is determined by the stoichiometry of the reaction, not simply by adding the volumes of reactants.
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Homework Statement


The reaction of 50 mL of H2 gas and 50 mL of N2 gas via the equation: 3H2 + N2 ---> 2NH3 will produce how many mL of product? A reaction of 25 mL of Hydrogen gas and 75 mL of Nitrogen gas? Assume that temperature and pressure are constant.


Homework Equations


Avogadro's Law


The Attempt at a Solution


I know that Volume of gases at STP are proportional to the moles of gas present, so the ratios are 3:1:2, and that i mole of ideal gas is 22.4 L. I'm not totally sure as to where to go from here. Is it kind of a limiting reagent because they give me the volumes of each reactant? Please help. Thanks!
 
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It is just a simple limiting reagent, with volumes instead of moles - but, as you have already mentioned, in this case moles and volume can be used interchangeably.
 
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Okay thank you. Well, I asked this question because of this problem: The reaction of 50 mL of chlorine gas with 50 mL of Ethylene gas Cl2 (g) + C2H4 (g) = C2H4Cl2 (g). How many mL of product will be produced? The answer is 50mL but I don't understand why. Since there is 50 mL of chorine and 50 mL of ethylene, shouldn't there be 100 mL of product? But instead, the answer is just 50 mL...
 
Take a look at the reaction equation. How many moles (total) on the left? How many moles on the right?
 
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