Hydrobromic acid dissolves solid iron according to the reaction: Fe(s) + 2 HBr(aq) → FeBr 2 (aq) + H 2 (g) What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock?

Hey everyone. Our question here is asking us to determine how many grams of hydrogen bromide are needed to completely dissolve 1.3 kg of pure iron. Looking at our reaction, we can see that it's unbalanced since we have two hydrogen in our product side and only one in our react inside. So we're going to need to balance this out by adding a two before our hydrogen bromine. And this works because now we also have to bro means in our product and in our react inside. Starting off with our 1.3 kg of pure iron, we're going to first convert this into g and so we know that per one kg we have 10 to the 3rd g. And now we want to convert our grams into moles of iron. And so looking at our periodic table, we can see that the Mueller massive iron is going to be 55.85 grams per mole. Now we want to relate this to our hydrogen bromide. Looking at our reaction, we can see that per one mole Of iron, we have two moles of hydrogen bromide and finally, we want to convert our hydrogen bromide instagrams and we're going to do so by calculating our molar mass. And when we do that, we find that hydrogen bromide Mueller mass is going to be 80. g per mole. So when do you calculate this out, we're going to end up with a value of 3766.62 g of hydrogen bromide, Which we can further simplify into 3.8 times 10 to the third grams of hydrogen bromide. And this is going to be our final answer. So I hope this made sense and let us know if you have any questions.

Ch.4 - Chemical Quantities & Aqueous Reactions

All textbooks

Tro 4th Edition

Ch.4 - Chemical Quantities & Aqueous Reactions

Problem 31a

Previous problem

Next problem

Chapter 4, Problem 31a

Hydrobromic acid dissolves solid iron according to the reaction:
Fe(s) + 2 HBr(aq) → FeBr₂(aq) + H₂(g)
What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock?

Verified step by step guidance

Identify the balanced chemical equation: \( \text{Fe(s)} + 2 \text{HBr(aq)} \rightarrow \text{FeBr}_2\text{(aq)} + \text{H}_2\text{(g)} \).

Determine the molar mass of iron (Fe) and hydrobromic acid (HBr). The molar mass of Fe is approximately 55.85 g/mol, and the molar mass of HBr is approximately 80.91 g/mol.

Calculate the number of moles of iron in the 3.2 g sample using the formula: \( \text{moles of Fe} = \frac{\text{mass of Fe}}{\text{molar mass of Fe}} \).

Use the stoichiometry of the balanced equation to find the moles of HBr needed. According to the equation, 1 mole of Fe reacts with 2 moles of HBr.

Convert the moles of HBr to grams using the formula: \( \text{mass of HBr} = \text{moles of HBr} \times \text{molar mass of HBr} \).

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the proportions of substances involved in a reaction. In this case, the stoichiometric coefficients from the balanced equation indicate that 2 moles of HBr are required for every mole of Fe, which is essential for calculating the mass of HBr needed.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles. For this problem, knowing the molar mass of HBr (approximately 80.91 g/mol) and Fe (approximately 55.85 g/mol) will help in determining how much HBr is needed to react with the given mass of iron.

Chemical Reaction Types

Understanding the type of chemical reaction is important for predicting the products and the behavior of reactants. The reaction between iron and hydrobromic acid is a single displacement reaction, where iron displaces hydrogen from HBr. Recognizing this helps in understanding the overall process and the stoichiometric relationships involved in the reaction.

Recommended video:

Guided course

02:25

Common Types of Alkane Reactions

Previous problem

Next problem

Related Practice

Textbook Question

Consider the balanced equation:

SiO₂(s) + 3 C(s) → SiC(s) + 2 CO(g)

Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.

1014

views

Textbook Question

Consider the balanced equation:

SiO₂(s) + 3 C(s) → SiC(s) + 2 CO(g)

1100

views

Textbook Question

Hydrobromic acid dissolves solid iron according to the reaction:

Fe(s) + 2 HBr(aq) → FeBr₂(aq) + H₂(g)

What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock? What mass of H₂ would the complete reaction of the iron bar produce?

471

views

Textbook Question

Sulfuric acid dissolves aluminum metal according to the reaction:

2 Al(s) + 3 H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3 H₂( g)

Suppose you want to dissolve an aluminum block with a mass of 15.2 g. What minimum mass of H₂SO₄ (in g) do you need? What mass of H₂ gas (in g) does the complete reaction of the aluminum block produce?

For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. a. Ba(s) + Cl2(g) → BaCl2(s) b. CaO(s) + CO2(g) → CaCO3(s) c. 2 Mg(s) + O2(g) → 2 MgO(s) d. 4 Al(s) + 3 O2(g) → 2 Al2O3(s)

Textbook Question

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

a. 2 K(s) + Cl₂(g) → 2 KCl(s)

b. 2 K(s) + Br₂(l) → 2 KBr(s)

c. 4 Cr(s) + 3 O₂(g) → 2 Cr₂O₃(s)

d. 2 Sr(s) + O₂(g) → 2 SrO(s)

3460

views

Hydrobromic acid dissolves solid iron according to the reaction:Fe(s) + 2 HBr(aq) → FeBr2(aq) + H2(g)What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock?

Verified Solution

Key Concepts

Stoichiometry

Molar Mass

Chemical Reaction Types

Hydrobromic acid dissolves solid iron according to the reaction:
Fe(s) + 2 HBr(aq) → FeBr₂(aq) + H₂(g)
What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock?