26. All atoms area. positively charged, with the number of protons exceeding the number of electronsb, negatively charged, with
the number of electrons exceeding the number of protonswith the number of protons equaling the number of electronsd. neutral, with the number of protons equaling the number of electrons. which is equal to thenumber of neutrons27. The particles that are found in the nucleus of an atom arec. protons and neutronsa, neutrons and electronsd. protons and electronsb. electrons only28. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to betrue?a. Protons. electrons, and neutrons are evenly distributed throughout the volume of the atom.b. The nucleus is made of protons, electrons, and neutrons.c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom.d. The nucleus is made of electrons and protons.29. The nucleus of an atom isa. the central core and is composed of protons and neutronsb. positively charged and has more protons than neutronsc. negatively charged and has a high densityd. negatively charged and has a low density
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<u>Answer:</u> The rate law for the reaction is
<u>Explanation:</u>
Rate law is the expression which is used to express the rate of the reaction in terms of the molar concentration of reactants where each term is raised to the power their stoichiometric coefficient respectively from a balanced chemical equation.
In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.
The chemical equation for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution follows:
The intermediate reaction of the mechanism follows:
<u>Step 1:</u>
<u>Step 2:</u>
<u>Step 3:</u>
As, step 2 is the slow step. It is the rate determining step
Rate law for the reaction follows:
......(1)
As, is not appearing as a reactant in the overall reaction. So, we apply steady state approximation in it.
Applying steady state approximation for from step 1, we get:
Putting the value of in equation 1, we get:
Hence, the rate law for the reaction is