Given: 2h2o2 → 2h2o + o2 structure of h2o2: h–o–o–h bond bond energy (kj/mol) o–h 459 o=o 494 o–o 142 based on the given bond energies, what is the enthalpy change for the chemical reaction? a. -352 kj b. -210 kj c. -176 kj d. -105 kj

B. - 210 kJ

Explanation:

∵ ΔHrxn = ∑(bond energies)products - ∑(bond energies)reactants.

The products:

The reactants:

∵ ΔHrxn = ∑(bond energies)products - ∑(bond energies)reactants.

∴ ΔHrxn = [2 (2 x (O–H bond energy) + (1 x (O=O bond energy)] - 2 [(2 x (O–H bond energy) + (1 x (O–O bond energy)] = [2 (2 x - 459 kJ/mol) + (1 x - 494 kJ/mol)] - 2 [(2 x 459 kJ/mol) + (1 x 142 kJ/mol)] = (- 2330 kJ) + (2120 kJ) = - 210 kJ.

yes they ca   is ur ansswerrr

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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