The enthalpy change for the following reaction is -136 kJ. Using bond energies, estimate the H-O...

The enthalpy change for the following reaction is -136 kJ. Using bond energies, estimate the H-O bond energy in H₂O₂(g).

H₂(g) + O₂(g) --> H₂O₂(g)

Expert Solution

Bond energies, kJ per mol
H-H 436

OH-OH = ?

O-O 142

O=O 498

deltaH = Total energy in breaking bond - Total energy in formation of bonds

Bond energy of H2 is H-H (+436) and O2 is O=O (+498) = 934 kJ /mol

H2O2 is H-O-O-H

Total energy in formation of bonds = (-2*BE of O-H bond)

hence -136 = 934 - (2*BE of OH bond +142)

hence BE of O-H bond is 464 kJ/mol

queen_honey_blossom answered 2 years ago

A scientist measures the standard enthalpy change for the following reaction to be -613.2 kJ :...

A scientist measures the standard enthalpy change for the following reaction to be -613.2 kJ : P4O10(s) + 6 H2O(l)-->4H3PO4(aq) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H3PO4(aq) is kJ/mol.

Calculate (using bond energies) the heat of reaction (per mole of CO, in KJ/Mol) for the...

Calculate (using bond energies) the heat of reaction (per mole of CO, in KJ/Mol) for the combustion of CO into CO2. Balance and do not round final answer Calculate (using bond energies) the heat of reaction (per mole of C2H2 in KJ/Mol) for the combustion of C2H2 into CO2 and water. Balance and do not round final answer

1. A chemical reaction at 304 K has an enthalpy change (delta-H) of -73.9 kJ/mol and...

1. A chemical reaction at 304 K has an enthalpy change (delta-H) of -73.9 kJ/mol and an entropy change (delta-S) of 161.6 kJ/mol. What is its Gibbs energy change, delta-G, in kJ/mol? Give the answer to one decimal place. 2.Use the thermodynamic data in your textbook to determine the temperature below which the following reaction is spontaneous. (Give the temperature in K, to the nearest degree.) 2SO2 (g) + O2 (g) -- 2SO3 (g) 3.What is the delta-G for the...

Use average bond energies to estimate the enthalpy changes of the following reactions: a. N2(g) +...

Use average bond energies to estimate the enthalpy changes of the following reactions: a. N2(g) + 3 H2(g) -> 2 NH3(g) b. N2(g) + 2 H2(g) -> H2NNH2(g) c. 2 N2(g) + O2(g) -> 2 N2O(g)

a) The standard enthalpy change for the following reaction is -270 kJ at 298 K. 2HCN...

a) The standard enthalpy change for the following reaction is -270 kJ at 298 K. 2HCN (g) --> 2 C(s, graphite) + H2 (g) + N2 (g) ΔH° = -270 kJ What is the standard enthalpy change for this reaction at 298 K? C (s, graphite) + 1/2 H2(g) + 1/2 N2(g) ---> HCN(g) _______ kJ

Calculate the change of enthalpy for: 4S + 6O2= 4SO3 Delta H= ___ kJ

A.) The standard enthalpy change for the following reaction is 359 kJ at 298 K. PbCl2(s)...

A.) The standard enthalpy change for the following reaction is 359 kJ at 298 K. PbCl2(s) ----> Pb(s) + Cl2(g) ΔH° = 359 kJ What is the standard enthalpy change for this reaction at 298 K? Pb(s) + Cl2(g) ----> PbCl2(s) __________ kJ B.) The standard enthalpy change for the following reaction is -602 kJ at 298 K. Mg(s) + 1/2 O2(g) ----> MgO(s) ΔH° = -602 kJ What is the standard enthalpy change for the reaction at 298 K? 2...

The standard enthalpy change for the following reaction is -170 kJ at 298 K. 2 Cu(s)...

The standard enthalpy change for the following reaction is -170 kJ at 298 K. 2 Cu(s) + 1/2 O2(g) Cu2O(s) ΔH° = -170 kJ What is the standard enthalpy change for the reaction at 298 K? 4 Cu(s) + O2(g) 2 Cu2O(s) A student determines the heat of dissolution of solid cobalt(II) chloride using a coffee-cup calorimeter of negligible heat capacity. When 1.33 g of CoCl2(s) is dissolved in 111.00 g of water, the temperature of the solution increases from...

For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 2.59 kJ...

For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 2.59 kJ at 25 oC and 4.73 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC.

#1. Estimate ΔH for the reaction using bond dissociation energies. Give your answer in kcal. C6H12O6...

#1. Estimate ΔH for the reaction using bond dissociation energies. Give your answer in kcal. C6H12O6 has five C−C bonds, seven C−H bonds, seven C−O bonds, and five O−H bonds. #2. Is the reaction exothermic or endothermic? #3. The following equation shows the conversion of aluminum oxide (from the ore bauxite) to aluminum: 2Al2O3(s)→4Al(s)+3O2(g), ΔH = +801.0 kcal ----> a. Is the reaction exothermic or endothermic?

Question