Which of the following would be the limiting reagent in the reaction shown below? There are 50 molecules of O2 and 50 molecules of H2.
2H2(g) + O2(g) ==> 2H2O(g)
Well, it seems like we've got ourselves a chemistry party! Now, let me just put on my lab coat and goggles... Oh wait, I'm a clown bot. I don't have those things. Anyway, to answer your question, we need to figure out which reactant is going to run out first and act as the limiting reagent here.
Now, if we look at the balanced chemical equation, we see that it takes 2 molecules of H2 and 1 molecule of O2 to make 2 molecules of H2O. Since we have 50 molecules of O2 and 50 molecules of H2, that means we have a balanced dance floor, my friend.
So, in this particular reaction, neither O2 nor H2 will be the limiting reagent because we have equal amounts. They will both be used up completely, and we're left with all 50 molecules of water (H2O) partying like there's no tomorrow.
So, grab a beaker and a dance partner, and let's get that reaction started! Woop woop!
To determine the limiting reagent, you need to compare the stoichiometric ratios of the reactants to the coefficients in the balanced chemical equation.
The balanced chemical equation for the reaction is:
2H2(g) + O2(g) ==> 2H2O(g)
From the equation, you can see that for every 2 molecules of H2, you need 1 molecule of O2 to react completely and produce 2 molecules of H2O.
Now, let's calculate the number of molecules of H2 and O2 available:
- H2: 50 molecules
- O2: 50 molecules
To find the limiting reagent, you can compare the ratio of the number of molecules of reactants to the required stoichiometric ratio in the balanced equation.
For H2:
50 H2 molecules * (1 O2 molecule / 2 H2 molecules) = 25 O2 molecules
For O2:
50 O2 molecules * (2 H2 molecules / 1 O2 molecule) = 100 H2 molecules
As you can see, the ratio of H2 to O2 is 25:1, and the ratio of O2 to H2 is 100:1. Therefore, the limiting reagent is O2 because it is in excess compared to the required stoichiometric ratio, while H2 is in the correct ratio.
To determine the limiting reagent in a chemical reaction, you need to compare the ratios of the reactants to the stoichiometric coefficients in the balanced equation. The reactant that produces the least amount of product, based on the balanced equation, is the limiting reagent.
In this case, the balanced equation is 2H2(g) + O2(g) ==> 2H2O(g).
To find the limiting reagent, you need to compare the number of molecules of each reactant with the stoichiometric coefficients. You have 50 molecules of both O2 and H2. Let's determine the limiting reagent by comparing the number of moles for each reactant.
The molar ratio between H2 and H2O is 2:2, meaning for every 2 moles of H2, you get 2 moles of H2O. Similarly, the molar ratio between O2 and H2O is 1:2, meaning for every 1 mole of O2, you get 2 moles of H2O.
First, convert the number of molecules to moles:
- For H2: 50 molecules x (1 mole/6.022 x 10^23 molecules) = (8.31 x 10^-23) moles
- For O2: 50 molecules x (1 mole/6.022 x 10^23 molecules) = (8.31 x 10^-23) moles
Now, compare the moles of each reactant to the stoichiometric coefficients in the balanced equation:
- For H2: (8.31 x 10^-23) moles H2 / 2 moles H2 = (4.16 x 10^-23) moles H2O
- For O2: (8.31 x 10^-23) moles O2 / 1 mole O2 = (8.31 x 10^-23) moles H2O
From this comparison, you can see that (4.16 x 10^-23) moles of H2O can be produced using the available moles of H2, while (8.31 x 10^-23) moles of H2O can be produced using the available moles of O2.
Since the reaction produces less H2O from the moles of H2, H2 is the limiting reagent in this reaction.