Considering the fact that the formation of a bond between two atoms is exothermic and is accompanied by an entropy decrease, explain why all chemical compounds decompose into individual atoms if heated to a high enough temperature. Select all that apply. Bond breaking always has a negative ΔΗ. Ο Bond breaking always has a positive ΔΗ. Breaking a bond into atoms always has a positive AS. Breaking a bond into atoms always has a negative AS. AG becomes negative at high temperature. O AG becomes positive at high temperature. This type of reaction becomes spontaneous at high temperature. This type of reaction is spontaneous at low temperature.

Considering the fact that the formation of a bond between two atoms is exothermic and is accompanied by an entropy decrease, explain why all chemical compounds decompose into individual atoms if heated to a high enough temperature. Select all that apply. Bond breaking always has a negative ΔΗ. Ο Bond breaking always has a positive ΔΗ. Breaking a bond into atoms always has a positive AS. Breaking a bond into atoms always has a negative AS. AG becomes negative at high temperature. O AG becomes positive at high temperature. This type of reaction becomes spontaneous at high temperature. This type of reaction is spontaneous at low temperature.

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

Calculate AH at 25°C for the reaction below. 4HCI(g) + O2(g) → 2C12(g) + 2H2O(g)
Use the table below to determine ΔH for the following reactionN 2H 4(g) + H 2O(g) ↔ NH 2OH(g) + NH 3(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 C≡C 835 C≡N 887 C≡O 1072 N=N 418 N=O 607 S=O (in SO2) 532 N≡N 942 O2 494 S=O (in SO3) 469
In the past, scientists were surprised that an endothermic process like the one in this lab, could be spontaneous. Which statement correctly describes why it seems like an endothermic process should not be spontaneous? Group of answer choices All endothermic processes create order in both the system and surroundings. Endothermic processes cause heat to flow from a cold object to a hot object. A process that spontaneously takes in energy seems to be analogous to a rock rolling up a hill. Endothermic processes become so cold that molecular motion stops.
Ethanol can be made from the fermentation of crops and has been used as a fuel additive to gasoline. C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Part B Calculate ΔrH∘ (The standard enthalpy of formation of liquid ethanol is −277.6 kJmol−1, of gaseous carbon dioxide is −393.5 kJmol−1, and of gaseous water is −241.8 kJmol−1.) Express your answer in kilojoules per mole to one decimal place.
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
How can bond energies be used to estimate ∆H for a reaction?
Decide whether the statement is True or False
1. Calculate the amount of heat absorbed when 35 g of carbon disulfide is formed. CS20) Cw+ 2S- AH= 89.3kJ
Question:Consider a hypothetical reaction A + B ⟶ C, where A and B are reactants and C is the product. The reaction is known to be exothermic and has a negative value for the enthalpy change (ΔH < 0). However, upon conducting the reaction in a laboratory setting, it is observed that the reaction does not occur spontaneously at room temperature (25°C). Explain this apparent contradiction and propose a possible explanation for this behavior
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol