SOLVE STEP BY STEP IN DIGITAL FORMAT Write the products of the following reactions, if there is more than one product, enter them and indicate which is the majority and if the compounds present stereochemistry, it must be entered appropriately. EXPLAIN THE REACTION MECHANISM STEP BY STEP 1) LDA 2) H Br LDA Br HCI N V H₂O Z.

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2) Consider the following reaction and associated rate law: X (g) + Y(g) → Z Rate = k[X] [Y] b Use the data in Table 1 in the following problems. Table 1 Reaction Data [X]。 (M) [Y]。 (M) Rate (M/s) 0.882 0.217 283. 07 0.882 0.451 624. 47 0.882 0.572 820.57 0.882 0.882 1308. 22 0.228 0.882 124.96 0.442 0.882 382. 56 0.67 0.882 804. 48

Suppose the concentration of a solute decays linearly along the length of a container according to c(x) = c0 - αc0x, where c0 is the concentration at x = 0. Calculate the thermodynamic force on the solute at 25 °C and at x = 10 cm and 20 cm given that the concentration falls to 1/2c0 when x = 10 cm. Hint: Start by finding the value of α.

The following sequence of steps has been proposed for the overall reaction between H2 and Br2 to form HBr:(1) Br2(g) 2Br(g)Write the overall balanced equation and show that the overall Qc is the product of the Qc’s for the individualsteps.

4. Which of the following best describes the timescales of fluorescence and phosphorescence? (b) Tfluorphos (d) there is no general trend Tfluor > Tphos Tfluor Tphos In 1-2 sentences, explain your reasoning:

6. Suppose that a gas phase reaction: 2A(g) 2B(g) +C(g) follows second order kinetics and goes to completion. If the reaction is allowed to proceed in a constant volume vessel at an initial pressure of 4 bar (only A is initially present). The total pressure of the reaction mixture at t= o is: * 4 bar 9 bar O 3 bar 6 bar

According to the nature or physical mechanism of separation, the separation process can be categorized into three main types. Write down in details what are the three main types.

7) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, 7) %3D %3D %3D and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 %3D %3D %3D %3D E) toward reactants because Q = 61 %3D

6. Five reaction mixtures containing equal concentrations of an enzyme are made up to the substrate concentrations [S] indicated in the table below and the initial rates of the reaction (V) are measured. The experiment is repeated with an enzyme inhibitor I present at 0.22 mM in each reaction mixture. (a) Determine Km for the substrate and K, for the inhibitor. (b) Can you say anything about the type of the inhibitor? [S], mM V (µmol/min) (no I) V (µmol/min) (+ 0.22 mM I) 0.1 28 17 0.15 36 23 0.2 43 29 0.5 65 50 0.75 74 61