The activation energy of a chemical reaction is the energy that must be released

Question

The activation energy of a chemical reaction is the energy that must be released from the mixture. Initiates the reaction must be removed from the mixture. Is the difference in the energies of the starting materials and products. Activates the catalyst. When a reaction is at equilibrium. All reaction stops. The reactions is no longer reversible. The products and reactants have the same energy content. No more reactants are converted to products. The reaction for the decomposition of PCI_S to chlorine and PIC_3 is shown below. PCI_s(g) PCI_3(g)+cI_2(g) If the equilibrium concentrations are [PCI_5]=1.0 M, [PCI_3]=0.10 M[CI_2]=0.10M, what is the value of the equilibrium constant? The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is K_c=2 times 10^11. This means that the reaction mixture at equilibrium is likely to consist of twice as much starting material as product. Twice as much product as starting material. An equal mixture of products and reactants/mostly starting materials. Mostly products. For the following reaction the equilibrium constant k_c is 2.0 at a certain temperature. If the concentration of both products is 0.10 M at equilibrium, what is the concentration of the starting material, 2NOBr? 2NOBr(g) 2NO(g)+Br_2(g)

Explanation / Answer

(1) B

(2) B. The forward and reverse reactions occur at the same rate.

(3) E.            Kc = (0.1*0.1) / 1.0 = 10 -2

(4) E mostly products

(5) E.        Kc = (0.12 * 0.1 )/ [NOBr]2 = 2

[NOBr]2 = 5 x 10 -4

[NOBr] = 2.2 x 10 -2

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