The reaction of limestone with hydrochloric acid is
CaCO3+2HCl⟶CaCl2+CO2+H2O
If the reaction produced 13.5 g CO2, how many grams of HCl reacted?
despertate help needed, 61.3 g is wrong
thank you!
find moles of CO2 ... 13.5 / 44.01
moles of HCl is twice moles CO2 ... 2 * 13.5 / 44.01
grams HCl equals moles times molar mass ... (27/44.01) * 36.46 g
thank you so much! that was correct!
Oh, don't be so bitter about it. Let's calculate this together, shall we?
We know that in the reaction 1 mole of CaCO3 reacts with 2 moles of HCl to produce 1 mole of CO2. The molar mass of CO2 is approximately 44 g/mol.
First, we need to calculate the number of moles of CO2 produced:
moles of CO2 = mass of CO2 / molar mass of CO2
moles of CO2 = 13.5 g / 44 g/mol ≈ 0.3068 mol
Since the ratio between CO2 and HCl is 1:2, we can say that 0.3068 mol of CO2 corresponds to 0.6136 mol of HCl.
Finally, we can calculate the mass of HCl:
mass of HCl = moles of HCl × molar mass of HCl
mass of HCl = 0.6136 mol × 36.46 g/mol ≈ 22.38 g
So, approximately 22.38 g of HCl reacted in this reaction.
To determine the mass of HCl reacted, we'll use the stoichiometry of the reaction.
From the balanced equation:
1 mole of CaCO3 reacts with 2 moles of HCl
First, let's convert the given mass of CO2 to moles.
The molar mass of CO2 is:
C = 12.01 g/mol
O = 16.00 g/mol (2 atoms)
Total = 44.01 g/mol
Using the formula:
moles = mass / molar mass
moles of CO2 = 13.5 g / 44.01 g/mol
moles of CO2 = 0.306 moles
Since the reaction produces CO2 and each mole of CO2 corresponds to 2 moles of HCl, we can determine the moles of HCl reacted.
moles of HCl = 0.306 moles CO2 x (2 moles HCl / 1 mole CO2)
moles of HCl = 0.612 moles
Now, we need to convert the moles of HCl to grams.
The molar mass of HCl is:
H = 1.01 g/mol
Cl = 35.45 g/mol
Total = 36.46 g/mol
Using the formula:
mass = moles x molar mass
mass of HCl = 0.612 moles x 36.46 g/mol
mass of HCl = 22.33 g
Therefore, 22.33 grams of HCl reacted in the given reaction.
To determine the number of grams of HCl that reacted in the given chemical reaction, we need to use stoichiometry.
First, we'll calculate the molar mass of CO2. Carbon (C) has a molar mass of 12.01 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol. Since there are two oxygen atoms in CO2, the molar mass of CO2 is:
(12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol
Now, we can use the balanced equation to create a conversion factor between CO2 and HCl. According to the balanced equation, for every 1 mole of CO2 produced, 2 moles of HCl react. This can be written as:
1 mole CO2 : 2 moles HCl
Using this conversion factor, we can convert grams of CO2 to moles of CO2, and then to moles of HCl. Finally, we can convert moles of HCl back to grams of HCl.
Step 1: Calculate the number of moles of CO2 produced
Given: 13.5 g CO2
Molar mass of CO2: 44.01 g/mol
Number of moles of CO2 = (given mass of CO2) / (molar mass of CO2)
Number of moles of CO2 = 13.5 g / 44.01 g/mol ≈ 0.3066 mol
Step 2: Convert moles of CO2 to moles of HCl using the stoichiometry from the balanced equation
According to the balanced equation, the ratio between moles of CO2 and moles of HCl is 1:2.
Number of moles of HCl = (number of moles of CO2) * (2 moles HCl / 1 mole CO2)
Number of moles of HCl = 0.3066 mol * (2 mol HCl / 1 mol CO2) ≈ 0.6132 mol
Step 3: Convert moles of HCl to grams of HCl
Molar mass of HCl: 36.46 g/mol
Mass of HCl = (number of moles of HCl) * (molar mass of HCl)
Mass of HCl = 0.6132 mol * 36.46 g/mol ≈ 22.38 g
Therefore, approximately 22.38 grams of HCl reacted.