Bond A-A B=B A-B The thalpy for the reaction below is -25 kJ: 2 A-A+B=B → 2 A-B-A a. Given the following bond energies, find the missing value. Bond Energy (kJ/mol) ?? 32. 46. b. Sketch a potential energy diagram for this reaction: roiny.

Bond A-A B=B A-B The thalpy for the reaction below is -25 kJ: 2 A-A+B=B → 2 A-B-A a. Given the following bond energies, find the missing value. Bond Energy (kJ/mol) ?? 32. 46. b. Sketch a potential energy diagram for this reaction: roiny.

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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Using the following bond enthalpies H-H F-F H-F 436 kJ/mol 157 kJ/mol 568 kJ/mol calculate AH for the reaction: H-H(g) + F-F(g) O-543 kJ 543 kJ 25.0 kJ O-1090 kJ O-25.0 kJ 2 H-F(g)
9. A 40.0 kg industrial calorimeter has an overall specific heat capacity of 1.00 J/ (g°C). Complete combustion of 1.00 g of hydrogen in this calorimeter causes a temperature increase of 3.54°C. Calculate the molar enthalpy of combustion for hydrogen from this evidence. (-286 kJ/mol)
Filin the blanks Answer. a. ENDOTHERMIC reaction kJ C. kJ -1 attachment Consider the following reaction: CH. (g) + 2 02 (g) → CO2 (g) + H20 (g) AH= -890 kJ a. Is the reaction endothermic or exothermic? b. How much heat is given off by the reaction of 3.5mol CH4? c. How much heat is given off by the reaction of 40.0 gram of O2?
Predict the enthalpy change for the reaction below, by combining reactions A-C. NO (g) + O (g)NO2 (g) ΔH=?? A. O3 (g)  3/2 O2 (g) ΔH=-142.3 kJ/mole B. O2 (g)  2 O (g) ΔH=495.0 kJ/mole C. NO (g) + O3 (g)  NO2 (g) + O2 (g) ΔH=-198.9 kJ/mole
6. Use the standard heat of formation AH to calculate the AH for the reaction: b. C2H4 (g) + C2H4(g)= 52 KJ H2 (g) → H2=0 KJ C₂H6 (g) C2H6(g) -84.7 KJ
Calculate the heat of reaction AH for the following reaction: 2 CH₂(g) + 30₂(g) 2 CO(g) + 4H₂O(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ mol olo Data For example, life of all No ToT walei. [-] Bond energies bond H-H H-F H-CI H-Br H-I H-C H-O H-N H-P H-S bond C-H energy (kJ/mol) 436 570 431 366 298 413 497 391 351 381 energy (kJ/mol) 413 bond O-H O-F O-CI O-Br O-I O-C O=C O=C 0-0 0=0 O-N O=N O=S bond N-H energy (kJ/mol) 497 215 234 210 213 385 532 1077 210 498 206 631 551 energy (kJ/mol) 391 bond F-F F-CI F-Br F-I CI-CI Cl-Br Cl-I Br-Br Br-I I-I bond S-H energy (kJ/mol) 159 261 280 272 243 219 211 194 179 152 energy (kJ/mol) 381
[Review Topics] The overall reaction in commercial heat packs can be represented as 4Fe(8) + 30₂(g) → 2Fe2O3 (8) AH = -1652 kJ a. How much heat is released when 4.44 mol iron is reacted with excess O2? kJ released b. How much heat is released when 1.58 mol Fe2O3 is produced? kl released c. How much heat is released when 1.73 g iron is reacted with excess O2? kJ released d. How much heat is released when 11.1 g Fe and 2.75 g O2 are reacted? Submit Answer kJ released Retry Entire Group [References] 9 more group attempts remaining Previous
Now consider the following set of reactions: 1. CO + O₂ CO₂, AH= -283 kJ/mol 2. CO₂ CO₂, AH=-393 kJ/mol
5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
8. 1.250 L of a 0.7601 mol/L Sodium Sulfide aqueous solution is mixed with 500.0 mL of a 0.7450mol/L aqueous solution of Lead (II) Nitrate. A. How much energy is absorbed or released by the reaction? B. If the reaction is carried out in a calorimeter whose constant is 14.60 kJ/°C and the solutions are initially at 21.000°C, what is the final temperature of the reaction solution on completion. Assume the heat capacity of the final solution is 4.200 J/g°C and that it has a density of 1.05 g/mL. Also assume that any solid formed does not absorb or give off heat.
Consider the reaction below with the indicated heats of formation. 2 N2O (g) + O2 (g) --> 4 NO (g) +82 kJ/mol +90 kJ/mol What is the energy absorbed or released when 1.0 mol of NO is produced? a. -196 kJ b. +23 kJ c. +49 kJ d. +90 kJ e. +196 kJ f. we cannot calculate the answer without knowing the heat of formation of oxygen gas
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