The image presents an educational stoichiometry problem. It involves a balanced chemical reaction and a table to calculate the changes in moles of reactants and products.### Problem Statement:"Consider the balanced chemical reaction below. What is the maximum number of moles of CO₂ that can be produced if 45.2 mol of C₂H₄O₂ and 76.5 mol of O₂ react?"**Balanced Chemical Equation:**\[ \text{C}_2\text{H}_4\text{O}_2(g) + 2 \, \text{O}_2(g) \rightarrow 2 \, \text{CO}_2(g) + 2 \, \text{H}_2\text{O}(g)\]### Instructions:"Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion."### Table Structure:- **Columns:** - C₂H₄O₂(g) - 2 O₂(g) - 2 CO₂(g) - 2 H₂O(g)- **Rows:** - Before (mol) - Change (mol) - After (mol)### Available Values:Below the table, there are several numerical options that can be used to fill in the table. These include values such as:0, 45.2, -45.2, 76.5, -76.5, 22.6, -22.6, 90.4, -90.4, 38.3, -38.3, 153, -153, 31.3, -31.3, 62.6, -62.6, 6.9, -6.9.Additionally, there is a "RESET" button to clear any entries and start over. This setup assists users in applying stoichiometric principles to calculate the limiting reactant and the maximum yield of products. ### Chemical Reaction Problem**Consider the balanced chemical reaction below:**\[ \text{C}_2\text{H}_4\text{O}_2(\text{g}) + 2 \text{O}_2(\text{g}) \rightarrow 2 \text{CO}_2(\text{g}) + 2 \text{H}_2\text{O}(\text{g}) \]**Problem Statement:**What is the maximum number of moles of CO\(_2\) that can be produced if 45.2 moles of C\(_2\)H\(_4\)O\(_2\) and 76.5 moles of O\(_2\) react?**Instructions:**- Based on your calculations, determine the maximum moles of CO\(_2\) that can be produced.- Enter your answer in the box provided: \[ \text{mol}_{\text{CO}_2} = \_\_\_\_ \text{ mol} \]#### Answer Choices:- 0- 45.2- 76.5- 22.6- 90.4- 38.3- 153- 62.6- 7.9- 31.3**Functionalities:**- Users can select their answer by clicking on one of the blue buttons with the mole values.- A "RESET" button is available to start over the problem-solving process if needed.This task is intended to assist students in applying stoichiometry to determine the limiting reactant and calculate the resulting product in a chemical reaction.

The maximum number of moles of CO2 that can be produced is nothing but the theoretical amount, that is the maximum amount that can be obtained from the reaction stoichiometry.To know this, one must know limiting reactant . Limiting reactant is the reactant that is consumed completely during the reaction. Using this we will find the maximum number of moles of CO2 produced.Given that,mol of C2H4O2 = 45.2 molmol of O2 = 76.5 mol Therefore, C2H4O2 is the limiting reactant (choose the reactant with less number of moles)Before :mol of C2H4O2 = 45.2 molmol of O2 = 76.5 molmol of CO2 = 0 mol (products are not formed yet )mol of H2O = 0 mol According to the reaction stoichiometry,1 mol of C2H4O2 gives 2 moles of CO2 45.2 mol of C2H4O2 gives ____mol of CO2 (45.2 mol C2H4O2) x (2 mol CO2 / 1mol C2H4O2) = 90.4 mol CO2 Change:mol of C2H4O2 = - 90.4 molmol of O2 = -90.4 molmol of CO2 = +90.4 mol = 90.4 molmol of H2O = + 90.4 mol = 90.4 mol just add up before and change to get afterAfter:mol of C2H4O2 = 45.2 mol - 90.4 mol = -45.2 molmol of O2 = -45.2 mol mol of CO2 = 0 mol+ 90.4 mol = 90.4 molmol of H2O = 90.4 molAccording to the reaction stoichiometry,1 mol of C2H4O2 gives 2 moles of CO2 45.2 mol of C2H4O2 gives ____mol of CO2 (45.2 mol C2H4O2) x (2 mol CO2 / 1mol C2H4O2) = 90.4 mol CO2 = molco2Therefore maximum number of moles of CO2 that can be produced are 90.4 mol

Science

Chemistry

Consider the balanced chemical reaction below. What is the maximum number of moles of CO2 that can be produced if 45.2 mol of C:H:O2 and 76.5 mol of O: react? C:H.O:(g) + 2 O:(g) → 2 CO:(g) + 2 H:O(g) 2 NEXT > Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion. C:H.O:(g) 2 0:(g) 2 CO:(g) 2 H:O(g) Before (mol) Change (mol) After (mol)

Consider the balanced chemical reaction below. What is the maximum number of moles of CO2 that can be produced if 45.2 mol of C:H:O2 and 76.5 mol of O: react? C:H.O:(g) + 2 O:(g) → 2 CO:(g) + 2 H:O(g) 2 NEXT > Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion. C:H.O:(g) 2 0:(g) 2 CO:(g) 2 H:O(g) Before (mol) Change (mol) After (mol)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

The image presents an educational stoichiometry problem. It involves a balanced chemical reaction and a table to calculate the changes in moles of reactants and products.

### Problem Statement:
"Consider the balanced chemical reaction below. What is the maximum number of moles of CO₂ that can be produced if 45.2 mol of C₂H₄O₂ and 76.5 mol of O₂ react?"

**Balanced Chemical Equation:**
\[ \text{C}_2\text{H}_4\text{O}_2(g) + 2 \, \text{O}_2(g) \rightarrow 2 \, \text{CO}_2(g) + 2 \, \text{H}_2\text{O}(g)\]

### Instructions:
"Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion."

### Table Structure:

- **Columns:**
- C₂H₄O₂(g)
- 2 O₂(g)
- 2 CO₂(g)
- 2 H₂O(g)

- **Rows:**
- Before (mol)
- Change (mol)
- After (mol)

### Available Values:
Below the table, there are several numerical options that can be used to fill in the table. These include values such as:
0, 45.2, -45.2, 76.5, -76.5, 22.6, -22.6, 90.4, -90.4, 38.3, -38.3, 153, -153, 31.3, -31.3, 62.6, -62.6, 6.9, -6.9.

Additionally, there is a "RESET" button to clear any entries and start over.

This setup assists users in applying stoichiometric principles to calculate the limiting reactant and the maximum yield of products.

### Chemical Reaction Problem

**Consider the balanced chemical reaction below:**

\[ \text{C}_2\text{H}_4\text{O}_2(\text{g}) + 2 \text{O}_2(\text{g}) \rightarrow 2 \text{CO}_2(\text{g}) + 2 \text{H}_2\text{O}(\text{g}) \]

**Problem Statement:**

What is the maximum number of moles of CO\(_2\) that can be produced if 45.2 moles of C\(_2\)H\(_4\)O\(_2\) and 76.5 moles of O\(_2\) react?

**Instructions:**

- Based on your calculations, determine the maximum moles of CO\(_2\) that can be produced.

- Enter your answer in the box provided:

\[ \text{mol}_{\text{CO}_2} = \_\_\_\_ \text{ mol} \]

#### Answer Choices:

- 0
- 45.2
- 76.5
- 22.6
- 90.4
- 38.3
- 153
- 62.6
- 7.9
- 31.3

**Functionalities:**

- Users can select their answer by clicking on one of the blue buttons with the mole values.
- A "RESET" button is available to start over the problem-solving process if needed.

This task is intended to assist students in applying stoichiometry to determine the limiting reactant and calculate the resulting product in a chemical reaction.

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