Determine the rate law for the following mechanism: CH3COOC2H5 + H2O → CH3COOC2H,* + OH (slow) CH3COOC2H6* → CH3COOH + C2H5* (fast) C2H5* + OH → C2H5OH (fast)

The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 20 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.7 ug/mL. What will the concentration be 40 minutes later? Round your answer to 2 significant digits. ug mL ?

The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 35 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.7 ug/mL. What will the concentration be 140 minutes later? Round your answer to 2 significant digits. ug mL

Which of the following statements is FALSE about molecularity of kinetic reactions? a) Multimolecular reactions rarely occurs in enzyme kinetics. b) Unimolecular reactions are defined as First-order reactions. c) Bimolecular reaction rates double when the reactant concentration doubles. d) The half-life of the bimolecular reaction depends on the concentration of the reactant. e) When the amount of one of two starting reactants is very low, it becomes the rate limiting reactant.

Please give handwritten

For the following reaction Mechanism write the overall reaction and write the rate law.  H3O++ I- → HI + H2O (fast)   H2O2 + HI → H2O + HOI (fast)  HOI + H3O++ I- →2H2O + I2 (slow)   I2 + I- → I3-(fast)

The following enzyme-catalyzed reaction follows zero-order kinetics. When the initial concentration of the reactant is 1.82 M and the rate constant is 1.43 M/min. What will be the remaining concentration in M of the reactant after 1.0 minute? Please report with 2 decimal places, without units. S--> P

1) NO(g)  + O2 (g)  ><  NO3 (g)  2) NO3(g) + NO(g)  > <   2NO2(g0   for the reaction mechanism given, what is the rate law for each elementary equation? What is the rate law for the overall reaction if the mechanism is correct?

Hypothetically, the reaction H2 + 2IC1→ I2+ 2HC1 is first order in [H2] and second order in [ICI]. Based on the first fast step given below and the fact that the second step is the slow step, propose a second-step mechanism, and show that it conforms to the experimentally determined reaction order. Assume that [I2] does not affect the reaction rate. H2 + 2ICI → I2 + 2HC1 Fast: 2ICI → I2 + 2Cl Slow:

For the reaction   2NO + Cl2  ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above            NO + Cl2  NOCl2     fast equilibriumNOCl2 + NO  2NOCl     slow            2NO  N2O2     fast equilibriumN2O2 + Cl2  2NOCl     slow            Cl2  2Cl     slowCl + NO  NOCl     fast            NO + Cl2  NOCl + Cl     slowCl + NO  NOCl     fast