k Os(g) O:(g) + O(g) Olg) + Oslg) - 20:(g)

Problem: Given the reaction H₂ (g) + N₂ (g) → NH3(g) (a) write the corresponding expressions for the reaction rate in terms of each reactant and product (hint: you may need to balance the equation first) (b) if oxygen gas is consumed at a rate of 4.96×10-5 M/s, what is the corresponding reaction rate and what is the rate of consumption of H₂ (g) and the rate of formation of NH3 (g)?

Organic Chemistry Loudon | Parise SEVENTH EDITION presented by Macmillan Learning The rate law for an addition reaction of bromine to an alkene is k[alkene][Br, 1? rate = The order of the alkene is The order of the bromine is: The overall kinetic order of the reaction is The units of the rate constant are: M-'s-! M-2s-1 M²s-1 ) s-1

Question: How can one derive the potential energy surface for a chemical reaction involving multiple transition states and intermediates using high-level quantum chemical methods, and how does this impact the reaction dynamics and overall reaction mechanism?

Describe how the catalytic mechanism of serine protease enzyme work, for amide hydrolysis

There are two factors associated with the Arrhenius Rate Constant Equation pre-exponential term, A. What are these factors and explain the meaning of each one?

The sucrose hydrolysis reaction is pseudo-first order, which means that...(1). The rate constant is practically 1.(2). The rate of transformation of sucrose into glucose and fructose is practically constant over time.(3). the concentrations of the products (glucose and fructose) will be approximately equal to 1 at the end of the reaction.(4). The plot of the logarithm of sucrose concentration versus time should be approximately a straight line.

Problem 2 Consider the following reaction between nitrogen dioxide gas and carbon monoxide gas 21 + 2H* + H2O2 → I2 + 2H20 (g) The experimentally determined rate law for this reaction is Rate = k [I"] [H2Oz]. The following mechanism has been proposed I + H2O2 → HOI + OH" HOI + I → OH" + I2 (g) Slow Fast H* + OH" → H2O Fast

9) If one reaction is a first-order reaction, this reaction should be a (a) simple reaction (b) unimolecular reaction (c) complex reaction (d) all of above are possible

Consider a reaction taking place in an aqueous solvent. The transition state for this reaction is capable of interacting more strongly with the aqueous solvent (through low potential energy interactions, including hydrogen-bonding) than with the reactant/ground state. Despite these strong potential energy interactions, the reaction rate is not significantly faster than the same reaction taking place in a non-polar solvent. Why? a)The transition enthalpy is unchanged by the aqueous solvent b)The transition Gibbs energy is reduced in the aqueous solvent c) The transition entropy is significantly negative in the aqueous solvated reaction d) The transition state internal energy is significantly negative in the aqueous solvated reaction d) none of the above