6.22 Consider the following mechanism for formation of a double helix from its strands A and B: A+B unstable helix (fast) unstable helix → stable double helix (slow) Derive the rate equation for the formation of the double helix and express the rate constant of the reaction in terms of the rate constants of the individual steps. What would be your conclusion if the pre-equilibrium assumption was replaced by the steady-state approximation?

6.22: In addition to solving the problem please give brief explanation for concepts and solution if able.

(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast

6.16: In addition to solving the problem please give brief explanation for concepts and solution if able.

Determine the Michaelis constant and the maximum velocity of the reaction without using excel/google sheets. Show how you find intercept (b)

The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.

The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF,=0,F4 step 2 slow: 0,F4- 02 + 2 F2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"[B]". , where '1' is understood (so don't write it if it's a 'l') for m, n etc. Rate =

Please answer all (4)

Consider the following proposed mechanismHBr + HBr ⇄ H2Br2(fast, equilibrium)HBr + R ⇄ ES(fast, equilibrium)H2Br2 +ES→P+2HBr(slow) (1a) What is the overall reaction? (1b) Identify all catalysts and intermediates in this reaction mechanism. (1c) What is the rate law derived from this mechanism? (1d) If the experimentally determined rate law is rate = k [HBr]3[R]1 what conclusion can be drawn? (1e) If the experimentally determined rate law is rate = k [HBr]2 what conclusion can be drawn? The equilibrium constant (KC) is 10.0 x 10-10 at

A mechanism involving the following elementary reactions has been proposed: 2 X (g) → X2 (g) (fast) X2 (g) +Y(g) = XY(g)+X(g) (slow) (8a) What is the reaction intermediate in this mechanism?   (8b) What overall rate law will this mechanism produce?