The reaction 2NO2(g) +  F2(g) à  2NO2F(g)  has a second order rate law, rate= k[NO2][F2]. Suggest a mechanism that is consistent with this rate law.

Consider the following multistep reaction: C+D = CD (fast) CD +D →CD2 (slow) CD2 + D→CD3 (fast) C+ 3D →CD3 (overall) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C3D]2 type k* [C]^3* [D]^2. • View Available Hint(s)

Determine the rate law for the formation of oxygen predicted by this mechanism. (Assume the steady-state approximation is valid for any reaction intermediates.) k₁ CIO + CIO + M (CIO)₂ → CIOO + Cl (CIO)2 + sunlight k3 C100 + M k4 →→ Cl + O₂ 2x (C1 + 03 net: 2 033 0₂ → CIO + O₂) (this reaction occurs twice in the mechanism)

(a) In the reaction mechanisms given, there are some chemical species which will get produced in one step and get consumed in the other step and that are not in reactants nor in products of the total reaction. Such species are known as intermediates of a reaction as the name suggests. Therefore, in mechanism 1, the intermediates are (CH3)2CHOH2+, Cl-, (CH3)2CH+. and in mechanism 2: (CH3)2CHOH2+, Cl-. These ions are neither reactants nor products of the given total equation.

The ozonization of pentene in carbon tetrachloride solution at 25 °C C5H10 +O3 → C5 H1003 is first order in C5H10 and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =

The reaction 2H2(g) + 2NO(g) ----> 2H2O(g) + N2(g) is a first-order in H2 and second order in NO. What is the rate law

The rate law for the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(g) is rate = K[NO]²[H₂] -1 If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 x 10-6 mol L-¹, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 X 9.56 5-1 mol L-¹5-1 L³ mol-³ s-1 3 L² mol-2 s-1 L mol-¹ S-1

NO2 + CO​NO + CO2 a -the rate law of this reaction

Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.

The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22011 + H20 → C;H1206 + CgH1206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C,,H,,0,1] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are 22 isomers.) 1.8x10-11 Arrhenius equation at this temperature). (Enter unrounded values.) (a) In neutral solution, k at 26°C and 8.5x10-11 -1 at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s), and the rate constant (in s) for this equation at 48°C (assuming the kinetics remain consistent with the activation energy 108 kJ/mol frequency factor rate constant X s-1 (b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10 M. How long (in s) will it take the solution to reach equilibrium…