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?
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?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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