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?

(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

8. (15 marks) A reaction is written as A(g) At 298 K, k₁ =0.21 s.1. k.₁=5×10 Pa¹·s¹. B(g) + C(g). k-1 As the temperature increased from 298 K to 310 K, the values of k₁ and k., are doubled (denoted as k2 and K.2). (1) Calculate the rate constant k at 298K; (2) Calculate the activation energy of both forward and reverse reactions; (3) Calculate AH and AU for the reaction at 298K; (4) Calculate the reaction time at the whole pressure reaching to 152 kPa. The initial pressure of A(g) is 100 kPa and the reaction temperature is 298 K.

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 =

Which of the following parameters would be different for a reaction carried out in the presence of a catalyst, compared with the same reaction carried out in the absence of a catalyst?

Writing the rate law implied by a simple mechanism Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 (CH,),CBr(aq) → (CH3),C"(aq) + Br (aq) 2 (CH3),C"(aq) + OH (aq) → (CH3),COH(aq) kz Suppose also k,»k,. That is, the first step is much faster than the second. olo Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k I Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k.2 for k = the reverse of the two elementary reactions in the mechanism. olo ||

Consider the following reaction mechanism. k1 C2H6O(aq) + HCl(aq) 5 C2H,O*(aq) + Cl(aq) k-1 (fast, reversible) k2 C2H¬O*(aq) + CI(aq) → C2H$CI(aq) + H2O(1) (slow) a) Write the overall reaction that is indicated by the mechanism. b) Are there any reaction intermediates? If so, identify them. c) Is there a catalyst? If so, identify it. d) What is the rate law for this mechanism?

The overall reactions A --> D occurs via the following mechanism with the given reaction energies and barriers for each step  Assume that a single step controls the rate of the reaction and that any steps preceding the rate-determining step can be considered quasi-equilibrium. What are the values for apparent activation barriers you would measure for the following.   i) Step 1 is the rate-determining step.   ii) Step 2 is the rate-determining step.