/ext/map/index.html?_con%3Dcon&external_browser%3D08launchUrl%=https%253/Chapter 6 HW # 2Saved3attempts leftCheck my workBe sure to answer all parts.1A mercury mirror forms inside a test tube as a result of the thermal decomposition of mercury(II)pointsoxide:2 HgO(s) →2 Hg(!) + O2(g)AH = 181.6 kJReferences(a) How much heat is needed to decompose 513 g of the oxide?kJ(b) If 607 kJ of heat is absorbed, how many grams of Hg form?x 100g Hg(Enter your answer in scientific notation.)McGrawHill< Prev3 of 15

Answered: Image /qna-images/answer/974bdf30-fe55-44e6-9204-b88c58ec35ef.jpg

Answered: 2 HgO(s) →2 Hg(!) + O2(g)

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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Ethanol, C2H6O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The heat of combustion of ethanol is 326.7 kcal/mol.The heat of combustion of 2-methylhexane, C7H16, is 1.150×103 kcal/mol. How much energy is released during the complete combustion of 446 grams of 2-methylhexane ?________ kcal Assuming the same efficiency, would 446 grams of ethanol provide more, less, or the same amount of energy as 446 grams of 2-methylhexane? _________. (more, less, or the same amount)
Use the set of three reactions shown below to answer the questions that follow.2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJN2(g) + O2(g) → 2NO(g) ΔH = +183 kJ If 35.5 g of NO g is reacted with excess oxygen, how much heat energy is produced?
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C,Ha (-1300. kJ/mol), CH (-1560. kJ/mol), and Ha (-286 kJ/mol), calculate AH for the reaction CH (s)+ 2H (s)C,He (g) 1- AH- kJ
Use the set of three reactions shown below to answer the questions that follow.2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJN2(g) + O2(g) → 2NO(g) ΔH = +183 kJ What mass of liquid water will be consumed during the production of 21200 J of energy assuming that there is excess nitrogen and oxygen?
In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH = 0.182 kJ/mol
(A) Write the balanced chemical equation for the formation of butane (C4H10). How does the potential energy change between the reactants and products in this reaction? (B) draw a potential energy diagram for this chemical reaction. (C) what is the relationship between energy changes and the breakdown and/or formation of covalent bonds? Explain your ideas in at least two sentences and remember to use vocabulary terms.
5. 'Н H H US LDA H₂O LDA H₂O
The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy, ΔH, changes sign when a process is reversed. Consider the reaction H2O(l)→H2O(g), ΔH =44.0kJ What will ΔH be for the reaction if it is reversed?
Using the equations N₂ (g) + 3 H₂ (g) → 2 NH₂ (9) AH° = -91.8 kJ/mol C(s) + 2 H₂(g) →→ CH₂ (g) AH° = -74.9 kJ/mol H₂(g) + 2 C(s) + N₂ (g) → 2 HCN (g) AH° = 270.3 kJ/mol - Determine the enthalpy (in kJ/mol) for the reaction CH₂(g) + NH₂(g) → HCN (g) + 3 H₂ (g).
According to the equation below, do the products have stronger or weaker bonds than the reactants? C (s) + 2H (g) → CH4 (g), ΔHrxn = -74.86 kJ/mol
What is the average bond energy in CO2? CO2(g) ΔH°f, = –393.5 kJ mol–1 CO(g) ΔH°f, = –110.5 kJ mol–1 C(g) ΔH°f, = +715 kJ mol–1 CO32–(aq) ΔH°f, = –676.3 kJ mol–1 O(g) ΔH°f, = +249.0 kJ mol–1 Question 5 options: 207 kJ mol–1 1607 kJ mol–1 804 kJ mol–1
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