Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O 2 ( g) → 2 Al 2 O 3 (s) a. 1 mol Al, 1 mol O 2 b. 4 mol Al, 2.6 mol O 2 c. 16 mol Al, 13 mol O 2 d. 7.4 mol Al, 6.5 mol O 2

Hello, everyone. Today we have the following problem. Write the balanced chemical equation for each reaction. So we have B Cobalt three oxide reacts with hydrogen gas to form solid Cobalt and liquid water. So what does that look like? So we would have our Cobalt three oxide which is a solid reacting with hydrogen gas, which is of course, a gas and this will react to form solid Cobalt and liquid water. So we look at this equation and we see that it is not quite balanced. Of course, if we compare Adams on both sides, we can see that on the left, we have two Cobalts, but on the right, we have one on the left, we have three oxygens, but on the right, we have two, we have one and then hydrogens, we have two on the left and two on the right. So we need to balance the Cobalts to do that. We need to add a two to the coefficient of cobalt. And our equation, we multiply that one by the two to get two. And the next we balance our oxygens. We see that we have three on the left and one on the right. So we need to add a coefficient of three to our water. Such that when we multiply that oxygen by three, we have three, but we also change the number of hydrogens. So instead of two, we now have three times two or six. So what number can we multiply our hydrogen gas on the left to get to six, three. So if you multiply that by three, we get six and now it's balanced. And if we look at our anti choices, we see that choice c best reflects this and with that, we have solved the problem overall, I hope this helped. And until next time.

Ch.4 - Chemical Quantities & Aqueous Reactions

All textbooks

Tro 4th Edition

Ch.4 - Chemical Quantities & Aqueous Reactions

Problem 38

Chapter 4, Problem 38

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O₂( g) → 2 Al₂O₃(s)
a. 1 mol Al, 1 mol O₂
b. 4 mol Al, 2.6 mol O₂
c. 16 mol Al, 13 mol O₂
d. 7.4 mol Al, 6.5 mol O₂

Verified step by step guidance

Identify the balanced chemical equation: 4 Al(s) + 3 O_2(g) → 2 Al_2O_3(s).

For each scenario, calculate the mole ratio of Al to O_2 based on the balanced equation, which is 4:3.

a. Calculate the amount of Al needed to react with 1 mol of O_2 using the ratio: (4 mol Al / 3 mol O_2) * 1 mol O_2.

b. Calculate the amount of O_2 needed to react with 4 mol of Al using the ratio: (3 mol O_2 / 4 mol Al) * 4 mol Al.

Compare the calculated amounts with the given amounts to determine the limiting reactant for each scenario.

Verified video answer for a similar problem:

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.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. To identify it, one must compare the mole ratio of the reactants used in the reaction to the coefficients in the balanced chemical equation.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine how much of each reactant is needed or how much product can be formed from given amounts of reactants.

Mole Ratio

Mole ratio is the ratio of moles of one substance to the moles of another substance in a balanced chemical equation. It is essential for converting between moles of reactants and products, allowing chemists to predict how much of each reactant is required or how much product will be produced in a reaction.

Recommended video:

Guided course

02:14

Neutron-Proton Ratio

Related Practice

Textbook Question

For each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. b. 2 HNO₃(aq) + Ca(OH)₂(aq) → 2 H₂O(l) + Ca(NO₃)₂(aq)

Textbook Question

Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br₂(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br₂

b. 1.8 mol Na, 1.4 Br₂

c. 2.5 mol Na, 1 mol Br₂

d. 12.6 mol Na, 6.9 mol Br₂

views

Textbook Question

Consider the reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) + 2 Cl₂(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl₂ form from the reaction mixture that produces the greatest amount of products?

Textbook Question

Consider the reaction: 2 CH₃OH(g) + 3 O₂(g) → 2 CO₂(g) + 4 H₂O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO₂ molecules form from the reaction mixture that produces the greatest amount of products?

Textbook Question

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.

Ti(s) + 2 Cl₂(g) → TiCl₄(s)

a. 4 mol Ti, 4 mol Cl₂

b. 7 mol Ti, 17 mol Cl₂

c. 12.4 mol Ti, 18.8 mol Cl₂

views

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O2( g) → 2 Al2O3(s)a. 1 mol Al, 1 mol O2b. 4 mol Al, 2.6 mol O2c. 16 mol Al, 13 mol O2d. 7.4 mol Al, 6.5 mol O2

Verified video answer for a similar problem:

Key Concepts

Limiting Reactant

Stoichiometry

Mole Ratio

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O₂( g) → 2 Al₂O₃(s)
a. 1 mol Al, 1 mol O₂
b. 4 mol Al, 2.6 mol O₂
c. 16 mol Al, 13 mol O₂
d. 7.4 mol Al, 6.5 mol O₂