An iron ore sample contains Fe 2 O 3 together with other substances. Reaction of the ore with CO produces iron metal: Fe 2 O 3 (s) + CO(g) → Fe(s) + CO 2 (g) (b) Calculate the number of grams of CO that can react with 0.350 kg of Fe 2 O 3 . (c) Calculate the number of grams of Fe and the number of grams of CO 2 formed when 0.350 kg of Fe 2 O 3 reacts.

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.3 - Chemical Reactions and Reaction Stoichiometry

All textbooks

Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 64b,c

Chapter 3, Problem 64b,c

An iron ore sample contains Fe₂O₃together with other substances. Reaction of the ore with CO produces iron metal: Fe₂O₃(s) + CO(g) → Fe(s) + CO₂(g) (b) Calculate the number of grams of CO that can react with 0.350 kg of Fe₂O₃. (c) Calculate the number of grams of Fe and the number of grams of CO₂ formed when 0.350 kg of Fe₂O₃ reacts.

Verified step by step guidance

First, we need to convert the mass of Fe2O3 from kilograms to grams because the molar mass of substances is usually expressed in grams per mole. We know that 1 kg = 1000 g, so multiply 0.350 kg by 1000.

Next, we need to calculate the number of moles of Fe2O3. The molar mass of Fe2O3 is approximately 159.69 g/mol. We can find the number of moles by dividing the mass of Fe2O3 by its molar mass.

From the balanced chemical equation, we can see that one mole of Fe2O3 reacts with one mole of CO. Therefore, the number of moles of CO that can react with Fe2O3 is the same as the number of moles of Fe2O3.

Now, we need to convert the number of moles of CO to grams. The molar mass of CO is approximately 28.01 g/mol. We can find the mass by multiplying the number of moles of CO by its molar mass.

Finally, the number of grams of CO that can react with 0.350 kg of Fe2O3 is the result from the previous step.

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 branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining how much of one substance is needed to react with a given amount of another.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule. In this problem, knowing the molar mass of Fe2O3 and CO is crucial for converting between grams and moles, which is necessary for stoichiometric calculations.

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It ensures the law of conservation of mass is upheld. In this case, the balanced equation for the reaction between Fe2O3 and CO provides the mole ratio needed to determine how much CO reacts with a specific mass of Fe2O3.

Recommended video:

Guided course

01:32

Balancing Chemical Equations

Related Practice

Textbook Question

The reaction between potassium superoxide, KO2, and CO2, 4 KO2 + 2 CO2¡2K2CO3 + 3 O2 is used as a source of O2 and absorber of CO2 in selfcontained breathing equipment used by rescue workers. (a) How many moles of O2 are produced when 0.400 mol of KO2 reacts in this fashion?

1945

views

Textbook Question

The reaction between potassium superoxide, KO2, and CO2, 4 KO2 + 2 CO2¡2K2CO3 + 3 O2 is used as a source of O2 and absorber of CO2 in selfcontained breathing equipment used by rescue workers. (b) How many grams of KO2 are needed to form 7.50 g of O2?

678

views

Textbook Question

Several brands of antacids use Al1OH23 to react with stomach acid, which contains primarily HCl: Al(OH)₃(s) + HCl(aq) → AlCl₃(aq) + H₂O(l) (b) Calculate the number of grams of HCl that can react with 0.500 g of Al(OH)₃. (c) Calculate the number of grams of AlCl₃ and the number of grams of H₂Oformed when 0.500 g of Al(OH)₃ reacts.

607

views

Textbook Question

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write the balanced chemical equation for this reaction. (b) How many grams of aluminum hydroxide are obtained from 14.2 g of aluminum sulfide?

2481

views

Textbook Question

Calcium hydride reacts with water to form calcium hydroxide and hydrogen gas. (a) Write a balanced chemical equation for the reaction.

1512

views

Textbook Question

Calcium hydride reacts with water to form calcium hydroxide and hydrogen gas. (b) How many grams of calcium hydride are needed to form 4.500 g of hydrogen?