What minimum volume of 14.0 M hydrochloric acid would be required to completely dissolve a 600.0 −g iron bar?
I'm getting around 2.3 L but it's saying it's incorrect...
hope this helps
1 OH- plus H+ = HOH or H2O One mole of OH- combines with one mole of H+ to make one mole of water. therefore .50 moles of OH- will combine with .50 moles of H+ to make .50 moles of H2O and the solution will be neutral with a pH of 7.
2. Balance the equation first. 2 HCl + Mg = MgCl2 plus H2(g)
Now get the l0 grams of Mg into moles. l0 grams Mg over 24 grams Mg/mole = .417 moles Mg
Now notice in the balanced equation that 2 moles of HCl reacts with one mole of Mg, therefore we need two times as many moles of HCl as we have of Mg.
2 times .417 moles Mg = .833 moles HCl needed
In any solution Moles solute = Molarity times volume in LITERS
switching this around Volume in Liters = Moles solute over Molarity
Volume HCl needed = .833 moles HCl over 7.0 Molar HCl = .119 Liters or 119 ml
3. Reaction balanced 2 Fe + 6HCl = 2 FeCl3 + 3 H2
Get the 450 grams of iron into moles first. 450 gms Fe over 56 grams Fe per mole = 8.04 moles Fe
Now use the balanced equation as a math platform. Write out the equation on a ;piece of paper.
Over the 2Fe enter 8.04 moles and below the same enter its coefficient of 2 moles
Now over the 6HCl enter X moles and below the same enter its coefficient of 6
Now cross multiply through the equation and solve for X moles of HCl I got 24.1 moles of HCl needed.
Moles HCl = Molarity times Volume in Liters
Volume in liters = Moles HCl over Molarity which = 24.1 moles HCl over 14.0 Molar HCl acid
which = 1.72 Liters HCl acid or 1720 ml. If if the pen held 5 ml of acid, it would have to be refilled about 344 times. No way this would fit into the pen.
The work done by Nick is interesting but it doesn't answer the question.
Fe + 2HCl ==> FeCl2 + H2
mols Fe = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Fe to mols HCl. That's mols HCl = twice mols Fe.
Now convert mols HCl to volume.
M HCl = mols HCl/L HCl.
You know M HCl and mols HCl, solve for L HCl. Convert to mL if desired. 2.3 L is way too large by a factor like 2000 time too large.
To find the minimum volume of 14.0 M hydrochloric acid required to dissolve a 600.0 g iron bar, we can use the balanced chemical equation between hydrochloric acid (HCl) and iron (Fe). The reaction is as follows:
Fe(s) + 2 HCl(aq) -> FeCl2(aq) + H2(g)
From the equation, we can see that it takes 2 moles of hydrochloric acid to react with 1 mole of iron.
First, we need to find the number of moles of iron in the 600.0 g bar. To do this, we'll divide the mass of iron by its molar mass.
Molar mass of iron (Fe) = 55.845 g/mol
Number of moles of Fe = Mass of Fe / Molar mass of Fe
Number of moles of Fe = 600.0 g / 55.845 g/mol = 10.732 mol
Since 2 moles of HCl react with 1 mole of Fe, we'll need twice the number of moles of hydrochloric acid.
Number of moles of HCl = 2 * Number of moles of Fe
Number of moles of HCl = 2 * 10.732 mol = 21.464 mol
Now, we can calculate the volume of 14.0 M hydrochloric acid needed using the definition of molarity:
Molarity (M) = Number of moles / Volume (in liters)
Volume (in liters) = Number of moles / Molarity
Volume (in liters) = 21.464 mol / 14.0 mol/L ≈ 1.533 L
So the minimum volume of 14.0 M hydrochloric acid required to completely dissolve a 600.0 g iron bar is approximately 1.533 liters.
To solve this problem, you need to use the concept of stoichiometry and balanced chemical equations. In this case, the balanced chemical equation for the reaction between hydrochloric acid (HCl) and iron (Fe) is:
Fe + 2HCl → FeCl2 + H2
From the balanced equation, we can see that 1 mole of iron reacts with 2 moles of hydrochloric acid. Moreover, the molarity (M) of the hydrochloric acid is given as 14.0 M, which means that it contains 14.0 moles of HCl in 1 liter (L) of solution.
To calculate the minimum volume of 14.0 M hydrochloric acid required, follow these steps:
Step 1: Convert the mass of the iron (600.0 g) to moles. To do this, divide the mass by the molar mass of iron. The molar mass of iron (Fe) is 55.845 g/mol.
600.0 g Fe × (1 mol Fe / 55.845 g Fe) = 10.73 mol Fe
Step 2: Since 1 mole of iron reacts with 2 moles of HCl, we need twice as many moles of HCl compared to iron. Therefore, multiply the moles of iron by 2.
10.73 mol Fe × 2 = 21.46 mol HCl
Step 3: Convert the moles of HCl to volume (in liters) using the molarity (M) of the hydrochloric acid.
21.46 mol HCl × (1 L HCl / 14.0 mol HCl) = 1.532 L HCl
Thus, the minimum volume of 14.0 M hydrochloric acid required to completely dissolve a 600.0 g iron bar is approximately 1.532 L (rounded to the nearest thousandth).
If you were getting a different answer, please double-check your calculations for errors or any conversions you may have missed.