Suppose the synthesis of ethylene dichloride proceeds by the following mechanism:step elementary reaction rate constant1 →+CH2CH2gCl2g+CH2CH2Cl+gCl−g k12 →+CH2CH2Cl+gCl−gCH2CH2Cl2g k2Suppose also k1 ≪ k2. That is, the first step is much slower than the second.Write the balanced chemical equation for the overall chemical reaction. Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.

Suppose the formation of nitrosyl chloride proceeds by the following mechanism:step elementary reaction rate constant1 →+NOgCl2gNOCl2g k12 →+NOCl2gNOg2NOClg k2Suppose also k1 ≪ k2. That is, the first step is much slower than the second.Write the balanced chemical equation for the overall chemical reaction. Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.

Suppose the formation of iodine proceeds by the following mechanism:step elementary reaction rate constant1 H2(g) + ICl(g) → HI(g) + HCl(g) k12 HI(g) + ICl(g) → I2(g) + HCl(g) k2Suppose also k1≫k2. That is, the first step is much faster than the second.Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. =k

Suppose the decomposition of nitryl chloride proceeds by the following mechanism:step elementary reaction rate constant1 NO2Cl(g) → NO2(g) + Cl(g) k12 Cl(g) + NO2Cl(g) → NO2(g) + Cl2(g) k2Suppose also k1≪k2. That is, the first step is much slower than the second.Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.

Suppose the formation of tert-butanol proceeds by the following mechanism:step elementary reaction rate constant1 →CH33CBraq+CH33C+aqBr−aq k12 →+CH33C+aqOH−aqCH33COHaq k2Suppose also k1 ≪ k2. That is, the first step is much slower than the second.Write the balanced chemical equation for the overall chemical reaction. Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.

Write the rate law for the following elementary reaction:CH2CH2(g) + Cl2(g) → CH2CH2Cl+(g) + Cl−(g)Use k1 to stand for the rate constant.