Consider the following stoichiometric reaction 2NO (g) + 2H2 (g) → N2 (g) + 2H2O (g) Write expressions for the reaction rate in terms of the rate of change for each reactant and product If the rate of consumption of H2 is 1e-6 mol/(L s), calculate the rate of production of N2

For the reaction 3O2(g) + 4NO(g) → 2N2O5(g) the rate of change in concentration of O2, Δ[O2]/Δ t = 0.48 mol/L*sec. What is the rate of change of NO and what is the rate of change of N2O5? Show your calculations.

Given- H2S (g) + O2 (g) → H2O (g) + S8 (g)-Write the expression of the rate in terms of the concentration of eachreactant and product over time.-If the rate of formation of S8 is 0.078 M/s, what is the rate ofdisappearance of H2S?

consider the reaction 2 H2 (g) + O2 (g) = 2H2O (g). Determine the rate in which H2O is formed

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Consider the following reaction:           2MnO4–(aq) + 10Br–(aq) + 16H3O+(aq) --> 2Mn2+(aq) + 5Br2(aq) + 24H2O(l)    In a reaction under a certain condition, if the rate for the formation of Br2 (D[Br2]/Dt) is 1.0 x 10–5 mol ‧ L–1 ‧ s–1, what is the rate for the disappearance of 2MnO4– (-D[MnO4–]/Dt) in mol ‧ L–1 ‧ s–1 ?    (A) 1.0 x 10–5                (B) 4.0 x 10–6                (C) 2.5 x 10–6                (D) 2.5 x 10–5

for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction

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The rate law for the reaction: NH4+ + NO₂ N₂ + 2H₂O is rate =k[NH4+][NO₂] It is found that the rate constant for this reaction is 3.05x10-4 M-1s-1. Calculate the rate of the reaction, including units, if [NH4*] is 0.265M and [NO₂] is 0.0803M. Attach File Browse Local Files

The mechanism for the reaction described by NO₂(g) + CO(g) → CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) NO₂(g) + NO(g) k₂ (2) NO3(g) + CO(g) → NO₂(g) + CO₂(g) Assuming that [NO] is governed by steady-state conditions, derive the rate law for the production of CO₂ (g). rate of CO₂ (g) production =