Find the limiting reactant for the initial quantities of reactants
2k(s) + Cl2(g)--> 2KCl(s)
1.8 mol K; 1 mol Cl2
I'm lost
See your post above.
To find the limiting reactant, you need to compare the stoichiometric ratios of the reactants to determine which one will be completely consumed first and limit the amount of product that can be formed.
In this case, we have 1.8 mol of potassium (K) and 1 mol of chlorine gas (Cl2).
First, we need to find the stoichiometric ratio of the reactants by looking at the balanced chemical equation:
2K(s) + Cl2(g) --> 2KCl(s)
According to the equation, the ratio of K to Cl2 is 2:1. This means that for every 2 moles of K, we need 1 mole of Cl2 to react completely.
Next, we compare the given amounts of reactants to the stoichiometric ratio. Divide the number of moles of each reactant by their stoichiometric coefficients:
For K: 1.8 mol K / 2 mol K = 0.9
For Cl2: 1 mol Cl2 / 1 mol Cl2 = 1
Based on the calculations, we can see that we have an excess of Cl2 (1 mol) compared to K (0.9 mol). The reactant that is completely consumed first is the limiting reactant, which is potassium (K) in this case. Therefore, the limiting reactant is K.
I hope this helps clarify the concept of finding the limiting reactant! Let me know if you have any further questions.