(d) The overall reaction A + B = C + D has a mechanism in elementary reactions given below, with rate coefficients indicated. X is a reactive intermediate. A + B X + C k1 X + B k2 X + C A + B k3 Derive an expression for the rate of formation of product D in terms of rate coefficients and reactant or product concentrations only. Simplify this expression under conditions of k2[B] >> k3[C] and k2[B] << k3[C].

Using Le Chatilier's Pronciple to predict whether adding some HClO (aq) causes the system to shift in the direction to products or reactions: HClO + H20= H20+ ClO

I want you to give me step by step solution and describe everything.

Using the graphic below as a reference, describe what happens to a reversible reaction as it attains equilibrium.

Please answer ALL parts of the question and show your work. Consider this reaction: N2(g) + 3H2(g)  <------>  2NH2(g)          H= -123kJ Describe how the concentration of H2 will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease, or not change? (a) The volume of the reaction chamber is decreased (b) Helium gas is added to the reaction chamber (c) The temperature is increased (d) N2 has is added to the reaction chamber

give handwritten answer-A+B -> X (kx) A+B -> Y (ky) A+B -> Z (kz) The substances A and B (with the initial concentration CA0=3 M and CB0=1 M) react in parallel (competing) reactions. What are the individual rate constants (kx,ky,kz) knowing that at the end of the reaction the proportions of the X,Y,Z are 8%, 91%, 1%, and after the first half hour the concentration of A becomes 2.2 M. The answer should be: kx = 1.73 x 10^(-3)   L/mol*s ky = 1.97 x 10^(-2)   L/mol*s kz = 2.17 x 10^(-4) L/mol*s

The overall gas phase reaction  3A --> B + 2C occurs via the following sequence of elementary steps 2A <--> I1 + B    k1,k-1 A + I1 --> 2I2        k2 I2 --> C               k3 1. write an expression for the overall reaction rate, r, in terms of the rate step 3, r3 2. using the answer from 1, obtain an expression for the reaction rate, r, in terms of rate constants and concentrations of reactants and products, only use PSSH.

Problem IX (10 p): Consider the isomerization of compound A from its cis to its trans isomer at 298 K, which is first order in both directions: ki cis-A = trans-A k2 The rate constant for the forward reaction is k1 = 4.2 × 10* s', and the rate constant for the reverse reaction is k2 = 2.1 × 10-ª s-1. %3D a) Calculate the equilibrium concentrations [cis-A]eq and [trans-A]eq, assuming that at time t= 0 all of A was in the cis-form, i.e., [cis-A]o = [A]o. (Hint: Use the fact that at any time, [cis-A] + [trans-A] = [A]o.) %3D b) Which reaction is spontaneous, the forward reaction or the reverse reaction? Provide your reasoning. Total /100 p

2. The gas-phase catalytic reaction A + B → C is believed to follow the mechanism below. Develop the rate law, assuming the adsorption of species A is the rate-limiting step. A+*A* A*+ BC* C* C+*

Consider the reaction CaCO3(s)→CaO(s)+CO2(g).Estimate ΔG∘ and if they will be spontaneous for this reaction at 1475K, 1100K, & 295K. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.)