AGO2 CH3OH(g) + 3 O₂(g) →2 CO₂(g) + 4H₂O(g)Use this information to complete the table below. Round each of your answers to the nearest kJ.The standard reaction free energyreaction3²-CH₂OH(g) + O₂(g)+ O₂(g)32CO₂(g) + 4H₂O(g)13CO₂ (8)₂(g) + H₂O(g) → — CH₂OH(g) +→==- 1378. kJ for this reaction:3CO₂(g) +43O₂(g)H₂O(g)22CH₂OH(g) + 30₂ (g)AGⓇ☐kJKJKJx10XS

Answered: Image /qna-images/answer/78135734-4e31-418d-a29b-0ff6d657bc35.jpg

The standard reaction free energy AGO = -1378. kJ for this reaction: 2 CH3OH(g) + 3O₂(g) →2 CO₂(g) + 4H₂O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction CO₂(g) + H₂O(g) → CH₂OH(g) + O₂(g) CH₂OH(g) + O₂(g) → CO₂(g) + H₁₂0 (g) - 2CO₂(g) + 4H₂O(g) → 2CH₂OH(g) + 30₂(g) AGº kJ x10 X S

The standard reaction free energy AGO = -1378. kJ for this reaction: 2 CH3OH(g) + 3O₂(g) →2 CO₂(g) + 4H₂O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction CO₂(g) + H₂O(g) → CH₂OH(g) + O₂(g) CH₂OH(g) + O₂(g) → CO₂(g) + H₁₂0 (g) - 2CO₂(g) + 4H₂O(g) → 2CH₂OH(g) + 30₂(g) AGº kJ x10 X S

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...

See similar textbooks

Similar questions

1. Use standard enthalpies of formation from the equation sheets or the back of your book to calculate H°rxn for this reaction. Then draw a Reaction Energy diagram for the reaction using "Reaction Progress" on the x-axis and "Potential Energy" on the y-axis. Label H°rxn, reactants and products on each diagram. 2 H2S(g) + 3 O2(g)  2 H2O(g) + 2 SO2(g) please help me to answer this question
In the following experiment, solid CaCl2 (M = 110.98 g/mol) is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔsolnH = ? kJ mol−1A 4.00 g sample of CaCl2 is added to a coffee-cup calorimeter containing 125 g of H2O. The initial temperature of water in the calorimeter is 22.0°C and the final temperature is 27.5°C. What is the enthalpy change for the dissolution reaction (ΔsolnH) in kJ per mole of CaCl2? Assume the specific heat capacity of the solution is the same as water (Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.
A 1.27-g sample of fumaric acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.50 °C. The calorimeter contains 1.01×103 g of water and the bomb has a heat capacity of 755 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of fumaric acid burned (kJ/mol).
Which one of the equations below is an endothermic reaction? A) SrO (s) + CO₂ (g) → SrCO₃ (s)∆H° = -234 kJ/mol B) H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C) H₂ (g) + C (s) + N₂ (g) → 2 HCN (g) ∆H° = 270.3 kJ/mol D) 2 K (s) + 2 H₂O (l) → 2 KOH (aq) + H₂ (g) ∆H° = -393.1 kJ/mol
Using the following information, calculate the ΔH∘rsn Δ H r s n ° for the reaction between ammonia gas and oxygen. 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l). NH3 -45.9 kJ/mol O2 0.0 kJ/mol NO 90.3 kJ/mol H2O -285.8 kJ/mol
13. Energy is stored in the body in adenosine triphosphate, ATP, which is formed by reaction between adenosine diphosphate, ADP, and dihydrogen phosphate ions. ADP3-(aq) + H2PO42-(aq) -----> ATP4-(aq) + H2O (l) ΔH° = 38 kJ Is the reaction endothermic or exothermic?
The reaction for the decomposition of potassium chlorate which is shown below. 2KClO3 (s) 3O2(g) + 2KCl(s) + 78 kJ What mass of KClO3 (s) would have decomposed to cause 250 mL of water in a calorimeter to change temperature from 20.00C to 55.00C.
Consider the following reaction: 2 Mg + O22 MgO AH xn=-1203 kJ Calculate the amount of heat (in kJ) associated with complete reaction of 97.2 grams of Mg. O-3862 kJ O-4812 kJ O-601.5 kJ -2406 kJ O-1203 kJ 13
Given the information below, what is ΔGrxn for the reaction CO(g) → C(s) + ½ O2(g)?C(s) + O2(g) → CO2(g) ΔGrxn = –394.4 kJCO(g) + ½ O2(g) → CO2(g) ΔGrxn = –257.2 kJ
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.
The value of ΔΔH° for the reaction below is -72 kJ. Therefore, ________ kJ of heat are released when 5.0 mol of HBrHBr is formed in this reaction.H2 (g) + Br2 (g) →→ 2HBr (g) ΔΔH° = -72 kJ
A student dissolves 13.8 g of ammonium chloride (NH4Cl) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water from 21.0 °C to 17.3 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) → NH(aq) + Cl¯ (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to t correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NH Cl.…