Greg reacts 5.0 moles of hydrochloric acid(HCL)with 1.5 moles of barium hydroxide(Ba(OH)2).Which reagent is the limiting reagent, and which is in excess?If the reagent runs to completion,how many moles of barium chloride(BaCl2)will be produced?
CAN SOMEONE PLEASE HELP ME.CHEMISTRY IS NOT MY FORTE,THANK-YOU
write the balanced equation
Ba(OH)2 + 2HCl >>> BaCl2 + 2H2O
for each mole of barium hydroxide, you need twice that of HCl. You have way to much of HCl.
I bet you get 1.5 moles of BaCl2
Just wanted to say thanx for the help Bob
To determine the limiting reagent, we need to compare the number of moles of each reactant to the stoichiometric ratio in the balanced equation.
The balanced equation for the reaction between hydrochloric acid (HCl) and barium hydroxide (Ba(OH)2) is:
2HCl + Ba(OH)2 → BaCl2 + 2H2O
From the given information, we have 5.0 moles of HCl and 1.5 moles of Ba(OH)2.
Now, let's calculate the moles of BaCl2 produced if the reaction goes to completion:
From the balanced equation, we can see that 2 moles of HCl react with 1 mole of Ba(OH)2 to produce 1 mole of BaCl2.
Therefore, the ratio of moles of HCl to Ba(OH)2 required for complete reaction is 2:1.
Since there are 5.0 moles of HCl and 1.5 moles of Ba(OH)2, we can determine the limiting reagent as follows:
- For HCl:
The ratio of moles needed to react with 1.5 moles of Ba(OH)2 is calculated as follows:
(1.5 moles Ba(OH)2) * (2 moles HCl / 1 mole Ba(OH)2) = 3.0 moles HCl
Since we only have 5.0 moles of HCl, which is more than the calculated 3.0 moles needed, HCl is in excess.
- For Ba(OH)2:
The ratio of moles needed to react with 5.0 moles of HCl is calculated as follows:
(5.0 moles HCl) * (1 mole Ba(OH)2 / 2 moles HCl) = 2.5 moles Ba(OH)2
Since we only have 1.5 moles of Ba(OH)2, which is less than the calculated 2.5 moles needed, Ba(OH)2 is the limiting reagent.
Therefore, Ba(OH)2 is the limiting reagent, and HCl is in excess.
To calculate the moles of BaCl2 produced, we can use the stoichiometric ratio from the balanced equation:
1 mole of Ba(OH)2 reacts to produce 1 mole of BaCl2.
Since we have 1.5 moles of Ba(OH)2, it will produce 1.5 moles of BaCl2.
Therefore, if the reaction goes to completion, 1.5 moles of BaCl2 will be produced.
To determine the limiting reagent and the excess reagent in a chemical reaction, we need to compare the stoichiometry (molar ratio) of the reactants to the balanced equation.
Let's start by writing the balanced equation for the reaction between hydrochloric acid (HCl) and barium hydroxide (Ba(OH)2):
HCl + Ba(OH)2 -> BaCl2 + H2O
According to the balanced equation, the molar ratio between HCl and Ba(OH)2 is 1:1. This means that for every 1 mole of HCl, we need 1 mole of Ba(OH)2 to react completely.
Given:
- Greg has 5.0 moles of HCl
- Greg has 1.5 moles of Ba(OH)2
Now, let's compare the number of moles of each reactant to the required stoichiometry to identify the limiting reagent:
For HCl:
Since the stoichiometry of HCl is 1:1, all 5.0 moles of HCl can react.
For Ba(OH)2:
Since the stoichiometry is 1:1, only 1.5 moles of Ba(OH)2 can react because we don't have enough to match the molar ratio.
Based on this calculation, the limiting reagent is Ba(OH)2 because it limits the amount of product that can be formed.
Now let's determine how many moles of BaCl2 will be produced when the reaction runs to completion:
Since the stoichiometry of BaCl2 in the balanced equation is also 1:1, the number of moles of BaCl2 produced will be equal to the number of moles of the limiting reagent, which is 1.5 moles of Ba(OH)2.
Therefore, when the reaction between Greg's 5.0 moles of HCl and 1.5 moles of Ba(OH)2 runs to completion, 1.5 moles of BaCl2 will be produced.