Consider the following reaction: A2 + B2 → 2AB ΔH = –321 kJ Bond energy (A2)...

Consider the following reaction: A2 + B2 → 2AB ΔH = –321 kJ Bond energy (A2) = 1/2AB Bond energy (B2) =393 kJ/mol. What is the numerical value for Bond energy (A2) ?

Solutions

Expert Solution

A2 + B2 → 2AB ΔH = –321 kJ

ΔH = ΔH A2 + ΔH B2 - 2* ΔH AB

-321 = ΔH A2 + 393 - 2* 2* ΔH A2 [ (A2) = 1/2AB ]

-321 = ΔH A2 + 393 - 4 ΔH A2

-321 = 393-3 ΔH A2

-3* ΔH A2 = -321-393

-3* ΔH A2 = -714

3* ΔH A2 = 714

ΔH A2 = 714/3 = 238KJ

The bond energy of A2 = 238KJ

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

If the bond energy for A2, B2, and A-B is 300, 200 and 100 kJ/mole, respectively,...

If the bond energy for A2, B2, and A-B is 300, 200 and 100 kJ/mole, respectively, the change in energy for the following reaction A2+B2=2A-B should be (in kJ): 500 300 -300 400 -400 Based on Coulomb’s law, when the K+ and Cl- ions are placed 10 nm apart, their interaction energy should be (in J): -2.31x10-19 -2.31x10-20 2.31x10-20 2.31x10-19 -2.31x10-18 Using the energy equation for the H atom, determine its energy when its principal quantum number n=∞ (in J):...

Consider the following reaction: PCl5 (g)⇄ PCl3 (g) + Cl2 (g) ΔH = 87.9 kJ/reaction For...

Consider the following reaction: PCl5 (g)⇄ PCl3 (g) + Cl2 (g) ΔH = 87.9 kJ/reaction For each of the following changes, indicate whether the reaction will proceed towards products, towards reactants, or have no net reaction to reestablish equilibrium. a. ___________ Temperature is increased b. ___________ The pressure is increased by decreasing the volume. c. ___________ The pressure is decreased by removing some PCl 5 (g) d. ___________ The pressure is increased by adding N2(g) e. ___________ Cl2(g) is removed...

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K...

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K • mol) ΔG°= 88.4 kJ This reaction: will proceed very slowly. will be spontaneous at low temperatures. has bonds in the products that are weaker than the reactants. may have fewer and more complicated molecules in the product.

Consider the following set of reactions: N2 + 2O2→N2O4 ,ΔH=−8 kJ/mol N2 + O2→2NO ,ΔH=180 kJ/mol...

Consider the following set of reactions: N2 + 2O2→N2O4 ,ΔH=−8 kJ/mol N2 + O2→2NO ,ΔH=180 kJ/mol The equations given in the problem introduction can be added together to give the following reaction: overall: N2O4→2NO + O2 However, one of them must be reversed, reaction 1: N2 + 2O2→N2O4 What is the enthalpy for reaction 1 reversed? reaction 1 reversed: N2O4→N2 + 2O2 Express your answer numerically in kilojoules per mole. What is the enthalpy for reaction 2?

For the reaction: 2A + B2 -> 2AB,+ H =+50.0 kJ a) Heat is released to...

For the reaction: 2A + B2 -> 2AB,+ H =+50.0 kJ a) Heat is released to the surroundings b) The standard enthalpy of formation for AB is 50.0 kJ c) The molecule AB contains less energy than A or B2 d) The reaction is endothermic e) The bond energy for each A-B bond is 50.0 kJ

The ΔH°rxn for the following reaction is −114.2 kJ/mol. At what temperature (in °C) would the...

The ΔH°rxn for the following reaction is −114.2 kJ/mol. At what temperature (in °C) would the Kc for the reaction be 6.4 x 109? 2NO(g) + O2(g) ↔ 2NO2(g) Kc = 4.9 x 105 at 184°C 271°C 183°C 110°C 74°C

Given the following thermodynamic data, calculate the lattice energy of CsF: ΔH°f[CsF(s)] = -554 kJ/mol ΔH°sublimation...

Given the following thermodynamic data, calculate the lattice energy of CsF: ΔH°f[CsF(s)] = -554 kJ/mol ΔH°sublimation [Cs] = 76.5 kJ/mol Bond energy [F-F] = 159 kJ/mol IE1 (Cs) = 376 kJ/mol EA1 (F) = -328 kJ/mol -1414 kJ/mol -1493 kJ/mol -714 kJ/mol -758 kJ/mol -837 kJ/mol

Consider the following reaction: 2 A + 3 B2 ⇌ A2B6 The initial concentrations of...

Consider the following reaction: 2 A + 3 B2 ⇌ A2B6 The initial concentrations of A and B2 are 0.245 M and 0.730 M, respectively, with no A2B6 initially present. When the reaction comes to equilibrium, the concentration of A2B6 is found to be 9.50×10−2 M. Part A What is the equilibrium concentration of A? Round your answer to 3 significant figures. Part B What is the equilibrium concentration of B2? Round your answer to 3 significant figures. Part...

Consider the following reaction at 321 K: 2 A (aq) + 1 B (aq) → 2...

Consider the following reaction at 321 K: 2 A (aq) + 1 B (aq) → 2 C (aq) + 1 D (aq) An experiment was performed with the following intitial concentrations: [A]i = 1.33 M, [B]i = 2.05 M, [C]i = 0.25 M, [D]i = 0.29 M. The reaction was allowed to proceed until equilibrium was reached at which time it was determined that [A] = 0.51 M. What was the maximum amount of work that could have been performed...

Part 1. Consider the following reaction at 298 K: 2H2(g)+O2(g)---->2H2O(g) ΔH=-483.6 kj/mol Calculate the following quantities:...

Part 1. Consider the following reaction at 298 K: 2H2(g)+O2(g)---->2H2O(g) ΔH=-483.6 kj/mol Calculate the following quantities: ΔSsys=____J(molxK) ΔSsurr=____J(molxK) ΔSuniv=____J (molxK) Part 2. For a particular reaction, ΔH = 168.1 kJ/mol and ΔS = -55.8 J/(mol·K). Calculate ΔG for this reaction at 298 K. Is this system spontaneaus as written, Is it in the reverse direction, Or is it at equilibrium?

Subjects