Considering the balanced chemical equation, 2NOBr(g) → 2NO(g) + Br2(g), at what rate are each product made for the three cases listed in (a)? The following reaction was found experimentally to be second-order in chlorine dioxide and first-order in hydroxide ions. −Δ[ClO2]/Δt = 0.115 mol / (L∙s) when [ClO2] = 0.100 mol/L and [OH−] = 0.0500 mol/L.2ClO2(aq) + 2OH−(aq) → ClO3−(aq) + ClO2−(aq) + H2O(l)Write the rate law for this reaction and give the value of its rate constant with proper units.How fast will chlorine dioxide be consumed if [ClO2] = 0.0100 mol/L and [OH−] = 0.0750 mol/L?

Chemical kinetics is the study of the reaction that how fast or slow a reaction is taking place. The…

Answered: The following reaction was found…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section14.4: Concentration-time Relationships: Integrated Rate Laws

Problem 14.8CYU: The catalyzed decomposition of hydrogen peroxide is first-order in [H2O2]. It was found that the...

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Considering the balanced chemical equation, 2NOBr(g) → 2NO(g) + Br₂(g), at what rate are each product made for the three cases listed in (a)?

The following reaction was found experimentally to be second-order in chlorine dioxide and first-order in hydroxide ions. −Δ[ClO₂]/Δt = 0.115 mol / (L∙s) when [ClO₂] = 0.100 mol/L and [OH⁻] = 0.0500 mol/L.

2ClO₂(aq) + 2OH⁻(aq) → ClO₃⁻(aq) + ClO₂⁻(aq) + H₂O(l)

Write the rate law for this reaction and give the value of its rate constant with proper units.
How fast will chlorine dioxide be consumed if [ClO₂] = 0.0100 mol/L and [OH⁻] = 0.0750 mol/L?

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