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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Chapter1: Chemical Foundations
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  1. 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)?

 

  1. 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)

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

 

 

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