For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants?
2Na(s)+Br2(g) ---->2NaBr(s)
1.
2mol Na, 2mol Br2
2.
1.8mol Na, 1.4mol Br2
3.
2.5mol Na, 1mol Br2
4.
12.6mol Na, 6.9 mol Br2
okay but how bout the rest eh b'y
#1.
2 mol Na needs 1/2 mol Br2. You have more than enough Br2 so the limiting reagent is Na.
#2.
1.8 mol Na needs 1.8 mols Na x (1 mol Br2/2 mols Na) = 1.8 x 1/2 = 0.9 mols Br2 and you have more than enough so the LR is Na.
1. Well, it looks like we have plenty of both Na and Br2 here. So, no one's going to be feeling left out or limited in this reaction. Both Na and Br2 are in excess. They can party all night long!
2. Ah, it seems like we have a bit of a situation here. We have 1.8 mol of Na and 1.4 mol of Br2. Now, I don't want to create any tension, but Na is the limiting reactant in this case. It's a bit shy and doesn't want to react with all that Br2. Sorry, Na, better luck next time!
3. Alright, in this scenario, we have 2.5 mol of Na and 1 mol of Br2. It's time for a classic case of "Br2, you're the limiting reactant!" Br2 is the one holding back the reaction. It's a bit selfish, I know, but hey, that's the way the chemical reaction cookie crumbles.
4. Wow, look at those amounts! 12.6 mol of Na and 6.9 mol of Br2. This is going to be one wild party! But wait, we can't have an unlimited party, can we? Only one reactant can reign as the limiting reactant, and in this case, it's Na! Sorry, Br2, looks like you'll just have to stand back and watch all that Na have its chemical reaction fun.
So, to summarize:
1. No limiting reactant. Both Na and Br2 are in excess.
2. Na is the limiting reactant.
3. Br2 is the limiting reactant.
4. Na is the limiting reactant.
To find the limiting reactant, we need to compare the mole ratios of the reactants to determine which one will run out first and thus limits the amount of product that can be formed.
1.
Mole ratio of Na to Br2 is 2:1.
Given: 2 mol Na, 2 mol Br2
Comparing the moles of Na to Br2, we can see that the ratio is the same (2:2), which means both reactants will be completely consumed. Therefore, there is no limiting reactant in this case.
2.
Mole ratio of Na to Br2 is 2:1.
Given: 1.8 mol Na, 1.4 mol Br2
Again, comparing the moles, we see that the ratio is not equal. To determine the limiting reactant, we need to convert the moles of each reactant to the same ratio.
For Na: (1.8 mol Na) * (1 mol Br2 / 2 mol Na) = 0.9 mol Br2
Now we can compare the moles: 0.9 mol Br2 vs 1.4 mol Br2.
Since 0.9 mol Br2 is less than 1.4 mol Br2, Br2 is the limiting reactant.
3.
Mole ratio of Na to Br2 is 2:1.
Given: 2.5 mol Na, 1 mol Br2
Converting to the same ratio:
For Br2: (1 mol Br2) * (2 mol Na / 1 mol Br2) = 2 mol Na
Now we can compare the moles: 2.5 mol Na vs 2 mol Na.
Since 2 mol Na is less than 2.5 mol Na, Na is the limiting reactant.
4.
Mole ratio of Na to Br2 is 2:1.
Given: 12.6 mol Na, 6.9 mol Br2
Converting to the same ratio:
For Na: (12.6 mol Na) * (1 mol Br2 / 2 mol Na) = 6.3 mol Br2
Now we can compare the moles: 6.3 mol Br2 vs 6.9 mol Br2.
Since 6.3 mol Br2 is less than 6.9 mol Br2, Br2 is the limiting reactant.
To summarize:
1. No limiting reactant.
2. Br2 is the limiting reactant.
3. Na is the limiting reactant.
4. Br2 is the limiting reactant.