text: # Problem: The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) NO(g) + CO2(g). The rate constant at 701 K is measured as 2.57 M-1s-1 and that at 895 K is measured as 567 M-1s-1.Use the value of the activation energy (Ea = 1.50 x 102 kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.
  
  ###### FREE Expert Solution
  
  This means we need to use the two-point form of the Arrhenius Equation:
  
  $\overline{){\mathbf{ln}}\frac{{\mathbf{k}}_{\mathbf{2}}}{{\mathbf{k}}_{\mathbf{1}}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}\left[\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\right]}$
  
  where:
  
  k1 = rate constant at T1
  
  k2 = rate constant at T
  
  Ea = activation energy (in J/mol)
  
  R = gas constant (8.314 J/mol∙K)
  
  T1 and T2 = temperature (in K).
  
  We first need to convert the activation energy from kJ/mol to J/mol:
  
  1 kJ = 103 J
  
  89% (488 ratings)
  ###### Problem Details
  
  The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) NO(g) + CO2(g). The rate constant at 701 K is measured as 2.57 M-1s-1 and that at 895 K is measured as 567 M-1s-1.
  
  Use the value of the activation energy (E= 1.50 x 102 kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.
explanation: The text extract contains a chemistry problem that involves calculating the rate constant of a reaction at a specific temperature using the Arrhenius equation. The problem provides the activation energy and rate constants at two different temperatures and asks to predict the rate constant at a third temperature. The extract also includes a detailed solution approach, indicating the steps to solve the problem.
distilabel_metadata.content: Evaluate the user given text extract and determine if it contains a math question and optionally and answer to this question.
  
  Output rules:
  
  1. Briefly describe the document and mention if it contains a question or a question and answer.
  2. Finalize the output with: Label: no-question,question,question-and-answer,multiple-question,multiple-question-and-answer
distilabel_metadata.role: system
distilabel_metadata.content: # Problem: The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) NO(g) + CO2(g). The rate constant at 701 K is measured as 2.57 M-1s-1 and that at 895 K is measured as 567 M-1s-1.Use the value of the activation energy (Ea = 1.50 x 102 kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.
  
  ###### FREE Expert Solution
  
  This means we need to use the two-point form of the Arrhenius Equation:
  
  $\overline{){\mathbf{ln}}\frac{{\mathbf{k}}_{\mathbf{2}}}{{\mathbf{k}}_{\mathbf{1}}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}\left[\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\right]}$
  
  where:
  
  k1 = rate constant at T1
  
  k2 = rate constant at T
  
  Ea = activation energy (in J/mol)
  
  R = gas constant (8.314 J/mol∙K)
  
  T1 and T2 = temperature (in K).
  
  We first need to convert the activation energy from kJ/mol to J/mol:
  
  1 kJ = 103 J
  
  89% (488 ratings)
  ###### Problem Details
  
  The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) NO(g) + CO2(g). The rate constant at 701 K is measured as 2.57 M-1s-1 and that at 895 K is measured as 567 M-1s-1.
  
  Use the value of the activation energy (E= 1.50 x 102 kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.
distilabel_metadata.role: user
distilabel_metadata.raw_output_q_a_detector_0: The text extract contains a chemistry problem that involves calculating the rate constant of a reaction at a specific temperature using the Arrhenius equation. The problem provides the activation energy and rate constants at two different temperatures and asks to predict the rate constant at a third temperature. The extract also includes a detailed solution approach, indicating the steps to solve the problem.
  
  Label: question-and-answer