Writing the rate law implied by a simple mechanism with an initial slow... Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +F₂ (g) → NO₂F (g) +F (g) 2 F(g) + NO₂ (g) → NO₂F (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = & rate constant k₁ k₂ 0-0 olo X 4 0/5 Izab

Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H, (g) + 2NO (g) → N,0 (g)+ H,0 (g) k1 H, (g) + N,0 (g) → N2 (g) + H20 (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates.

The rate constant for this second‑order reaction is 0.630 M−1⋅s−1at 300 ∘C.   A⟶products   How long, in seconds, would it take for the concentration of A to decrease from 0.920 M to 0.290 M?   t= ? s

X, + Y2 - X,Y2 rate = K[X,] A reaction and its experimentally determined rate law are represented above. A chemist proposes two different possible mechanisms for the reaction, which are given below. Mechanism 1 X, - 2 X (slow) X + Y, - XY, (fast) Mechanism 2 X, -- 2 X (slow) X + Y2 + XY + Y (fast) X + XY, - X,Y, (fast) X+ XY -- X,Y (fast) X,Y + Y → X,Y, (fast) Based on the information above, which of the following is true? Both mechanism 1 and mechanism 2 are consistent with the rate law. Only mechanism 2 is consistent with the rate law. Only mechanism 1 is consistent with the rate law. Neither mechanism 1 nor mechanism 2 is consistent with the rate law.

Suppose the formation of iodine proceeds by the following mechanism: step elementary reaction 1 H₂(g) + IC1 (g) → HI(g) + HC1 (g) k₁ 2 HI (g) + IC1 (g) → I₂ (g) + HCl (g) k₂ Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant

The generic reaction     2 A   →   products     follows zero-order kinetics with a rate constant of 0.00628 M/s.  What is the half-life of substance A if its original concentration is 2.23 M? Be sure to enter a unit with the answer.

Initialte data a centain empera - fat rafe tuse is given in He table forr the the fable for the followingreactim. Determine the pate constont, Ko नाप the value and emits of

The rate constant for this first‑order reaction is 0.0210 s−1 at 400 ∘C. A⟶products After how many seconds will 22.9% of the reactant remain?

Direction:Express the rate of the following chemical reactions in terms of the change in concentration of the reactants or products. 1.2NO2(g)→N2 (g)+ 202 (g) 2.N2 (g)+ 3H2 (g)→2NH3 (g) 3.2C4H10 (g)+ 1302 (g)→8CO2 (g)+ 10H2O(g)

At a certain temperature the rate of this reaction is second order in ClCH2CH2Cl with a rate constant of ·0.0543M−1s−1: →ClCH2CH2Clg+CH2CHClgHClg Suppose a vessel contains ClCH2CH2Cl at a concentration of 0.710M. Calculate the concentration of ClCH2CH2Cl in the vessel 210. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M