Write A Balanced Equation For The Combustion Of C9H20(l) (nonane ...

This problem has been solved by verified expert Dinesh Singh 100% free to try - get full access instantly Start Free Trial

Question

Write a balanced equation for the combustion of C9H20(l) (nonane) -- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol 1. What is the standard heat of reaction (ΔH°) for the combustion reaction of C9H20(l)? 2. Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane. (Assume standard state conditions and 298 K for all reactants and products.) Write a balanced equation for the combustion of C9H20(l) (nonane) -- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol 1. What is the standard heat of reaction (ΔH°) for the combustion reaction of C9H20(l)? 2. Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane. (Assume standard state conditions and 298 K for all reactants and products.) Show more…

Added by Enrique M.

Chemistry: Structure and Properties Nivaldo Tro 2nd Edition

Step 1

Step 1: Write the balanced chemical equation for the combustion of C9H20(l): C9H20(l) + 14O2(g) -> 9CO2(g) + 10H2O(l) Show more…

Show all steps

Please give Ace some feedback

Your feedback will help us improve your experience

Submit Thanks for your feedback! Write a balanced equation for the combustion of C9H20(l) (nonane) -- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol 1. What is the standard heat of reaction (ΔH°) for the combustion reaction of C9H20(l)? 2. Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane. (Assume standard state conditions and 298 K for all reactants and products.) Play audio Feedback Powered by NumerAI

Dinesh Singh and 81 other Chemistry 101 educators are ready to help you.

Ask a new question

Key Concepts

Key Concept Premium Feature Explore the core concept behind this problem. View Video View Video Key Concept Premium Feature Explore the core concept behind this problem. Your browser does not support the video tag. Close Try it Now

Recommended Videos

Enthalpy of Combustion - Alkanes Write a balanced equation for the combustion of C9H20(l) (nonane) - i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol What is the standard heat of reaction (ΔH°) for the combustion reaction of C9H20(l)? 1 pt Calculate the difference, ΔH - ΔE = Δ(PV) for the combustion reaction of 1 mole of nonane. (Assume standard state conditions and 298 K for all reactants and products.)

Adi S.

For the unbalanced combustion reaction shown, $1 \mathrm{~mol}$ of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH},$ releases $1370 \mathrm{~kJ}:$ $$ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} $$ (a) Write a balanced equation for the combustion reaction. (b) What is the sign of $\Delta H$ for this reaction? (c) How much heat (in kilocalories) is released from the combustion of $5.00 \mathrm{~g}$ of ethanol? (d) How many grams of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ must be burned to raise the temperature of $500.0 \mathrm{~mL}$ of water from $20.0^{\circ} \mathrm{C}$ to $100.0^{\circ} \mathrm{C} ?$ (The specific heat of water is $4.184 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}$ See Section 1.11.) (e) If the density of ethanol is $0.789 \mathrm{~g} / \mathrm{mL},$ calculate the combustion energy of ethanol in kilojoules/milliliter.

The equation for the combustion of $\mathrm{CH}_{4}$ (the main component of natural gas) is shown below. How much heat is produced by the complete combustion of $237 \mathrm{g}$ of $\mathrm{CH}_{4} ?$ $$\begin{array}{r}\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \\&\Delta H_{\mathrm{rxn}}=-802.3 \mathrm{kJ} \end{array}$$

Recommended Textbooks

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition 1,646 solutions

Chemistry The Central Science

Theodore L. Brown 14th Edition 1,925 solutions

Chemistry

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste 10th Edition 1,223 solutions

Transcript

00:01 Question is right of balance equation for the competition of this. 00:04 We have to add down the balance chemical elevation for the combustion of this reaction. 00:10 C9h20. 00:11 C9h20 means alken... Need help? Use Ace Ace is your personal tutor. It breaks down any question with clear steps so you can learn. Start Using Ace Ace is your personal tutor for learning Step-by-step explanations Instant summaries Summarize YouTube videos Understand textbook images or PDFs Study tools like quizzes and flashcards Listen to your notes as a podcast

What our educators say

25992 Students Helped in Chemistry 101 “Numerade has a great goal - to increase people's educational levels all around the world. Educators do not complete student's personal homework tasks. We create video tutorials that may be used for many years in the future.” Dr. Mei Lin Chen PhD in Chemistry 101

44601 Students Helped in Chemistry 101 "The format has forced me to think about what knowledge is needed by the student to solve a problem and present it concisely and understandably within the time constraint of the video." Dr. Emily Green PhD in Chemistry 101

30417 Students Helped in Chemistry 101 “Explaining topics while I make Numerade videos has helped me deepen my own understanding and come up with new ways to help my students grasp concepts while I'm teaching.” Professor Jonathan Reed Master's in Chemistry 101

Get step-by-step video solutionfrom top educators Start your free 7-day trial, Sign up now. Continue with Facebook Continue with Apple Continue with Clever or Name Email Password Create Account By creating an account, you agree to the Terms of Service and Privacy Policy Already have an account? Log In A free answerjust for you

Watch the video solution with this free unlock.

View the Answer

Log in to watch this video ...and 100,000,000 more!

EMAIL

PASSWORD

Log in OR Continue with Facebook Continue with Apple Continue with Clever Don't have an account? Sign Up