Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 18

Consider the equation \(2 A+B \longrightarrow A_{2} B .\) If you mix 1.0 mole of \(A\) with 1.0 mole of \(B,\) what amount (moles) of \(A_{2} B\) can be produced?

Short Answer

Expert verified
When 1.0 mole of A and 1.0 mole of B are mixed, the limiting reactant is A. Using stoichiometry, 0.5 moles of A2B can be produced from the given amounts of reactants.

Step by step solution

01

Identify the limiting reactant

Given the balanced equation: \[ 2A + B \longrightarrow A_{2}B \] We have to identify the limiting reactant, which is the reactant that will run out first during the reaction and determine the amount of product formed. First, let's calculate the mole ratios of reactants A and B. In the balanced equation, for every 2 moles of A, 1 mole of B is consumed. Mole ratio A:B = 2:1
02

Calculate the moles of reactant required based on the balanced equation

We have 1.0 mole of A and 1.0 mole of B, let's calculate how much of each reactant required based on mole ratios: Moles of A required for 1 mole of B = (2 moles of A)/(1 mole of B) * (1 mole of B) = 2 moles of A Since, we only have 1.0 mole of A (which is less than the required 2 moles), A is the limiting reactant.
03

Use stoichiometry of limiting reactant to calculate the moles of A2B

Using stoichiometry, we can find out the amount of A2B that can be produced. From the balanced equation, when 2 moles of A reacts with 1 mole of B, 1 mole of A2B is produced. Moles of A2B formed = (1 mole of A2B)/(2 moles of A) * (1.0 mole of A) = 0.5 mole of A2B So, 0.5 moles of A2B can be produced from the given amounts of reactants A and B.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) $$ a. What is the maximum mass of ammonia that can be produced from a mixture of \(1.00 \times 10^{3} \mathrm{g} \mathrm{N}_{2}\) and $5.00 \times 10^{2} \mathrm{g} \mathrm{H}_{2} ?$ b. What mass of which starting material would remain unreacted?

Boron consists of two isotopes, 10 \(\mathrm{B}\) and 11 \(\mathrm{B}\) . Chlorine also has two isotopes, 35 \(\mathrm{Cl}\) and 37 \(\mathrm{Cl}\) . Consider the mass spectrum of \(\mathrm{BCl}_{3}\) . How many peaks would be present, and what approximate mass would each peak correspond to in the BCl_ mass spectrum?

A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 \(\mathrm{mg}\) of the compound yields 16.01 \(\mathrm{mg}\) \(\mathrm{CO}_{2}\) and 4.37 \(\mathrm{mg} \mathrm{H}_{2} \mathrm{O}\) . The molar mass of the compound is 176.1 \(\mathrm{g} / \mathrm{mol} .\) What are the empirical and molecular formulas of the compound?

Glass is a mixture of several compounds, but a major constituent of most glass is calcium silicate, \(\mathrm{CaSiO}_{3}\) . Glass can be etched by treatment with hydrofluoric acid; HF attacks the calcium silicate of the glass, producing gaseous and water-soluble products (which can be removed by washing the glass). For example, the volumetric glassware in chemistry laboratories is often graduated by using this process. Balance the following equation for the reaction of hydrofluoric acid with calcium silicate. $$ \mathrm{CaSiO}_{3}(s)+\mathrm{HF}(a q) \longrightarrow \mathrm{CaF}_{2}(a q)+\mathrm{SiF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l) $$

Lanthanum was reacted with hydrogen in a given experiment to produce the nonstoichiometric compound \(\mathrm{LaH}_{2.90}\) Assuming that the compound contains \(\mathrm{H}^{-}, \mathrm{La}^{2+},\) and \(\mathrm{La}^{3+},\) calculate the fractions of \(\mathrm{La}^{2+}\) and \(\mathrm{La}^{3+}\) present.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free