8. What is [NO] and [CO₂] (in M to two deci at 227 °C if the initial concentrations of each reactant is 1.25 M? Explain the validity of final answer using chemical intuition. NO₂(g) + CO(g) = NO(g) + CO₂(g) Hrxn = 1-1 K(227 °C) = 6.9x105 A: [NO] = 1.25; [CO₂] = 1.25 -224.09 kJ mol
8. What is [NO] and [CO₂] (in M to two deci at 227 °C if the initial concentrations of each reactant is 1.25 M? Explain the validity of final answer using chemical intuition. NO₂(g) + CO(g) = NO(g) + CO₂(g) Hrxn = 1-1 K(227 °C) = 6.9x105 A: [NO] = 1.25; [CO₂] = 1.25 -224.09 kJ mol
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Title: Chemical Equilibrium and Concentration Calculations**
**Question:**
8. What is [NO] and [CO₂] (in M to two decimal places) at equilibrium for the following reaction at 227 °C if the initial concentrations of each reactant is 1.25 M? Explain the validity of your final answer using chemical intuition.
**Chemical Reaction:**
\[ \text{NO}_2(g) + \text{CO}(g) \rightleftharpoons \text{NO}(g) + \text{CO}_2(g) \]
- \(\Delta H_{rxn} = -224.09 \, \text{kJ mol}^{-1}\)
- \(K_c (227 \, °C) = 6.9 \times 10^5\)
**Assumption:**
- Initial concentrations: \([NO] = 1.25 \, \text{M}\); \([CO_2] = 1.25 \, \text{M}\)
**Explanation:**
To find the equilibrium concentrations, apply the equilibrium constant expression:
\[ K_c = \frac{[\text{NO}][\text{CO}_2]}{[\text{NO}_2][\text{CO}]} \]
This exercise involves setting up an ICE table (Initial, Change, Equilibrium) to solve for equilibrium concentrations when initial concentrations are known, and using the equilibrium constant to verify the solution.
**Note:** The reaction is exothermic, indicated by the negative enthalpy change (\(\Delta H_{rxn}\)). This might influence the temperature effect on the equilibrium position.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8e77b376-6a5c-4963-870c-f49a6e984799%2Ffadbf780-1989-4af1-81af-78854b17d997%2Fj5m1tg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Chemical Equilibrium and Concentration Calculations**
**Question:**
8. What is [NO] and [CO₂] (in M to two decimal places) at equilibrium for the following reaction at 227 °C if the initial concentrations of each reactant is 1.25 M? Explain the validity of your final answer using chemical intuition.
**Chemical Reaction:**
\[ \text{NO}_2(g) + \text{CO}(g) \rightleftharpoons \text{NO}(g) + \text{CO}_2(g) \]
- \(\Delta H_{rxn} = -224.09 \, \text{kJ mol}^{-1}\)
- \(K_c (227 \, °C) = 6.9 \times 10^5\)
**Assumption:**
- Initial concentrations: \([NO] = 1.25 \, \text{M}\); \([CO_2] = 1.25 \, \text{M}\)
**Explanation:**
To find the equilibrium concentrations, apply the equilibrium constant expression:
\[ K_c = \frac{[\text{NO}][\text{CO}_2]}{[\text{NO}_2][\text{CO}]} \]
This exercise involves setting up an ICE table (Initial, Change, Equilibrium) to solve for equilibrium concentrations when initial concentrations are known, and using the equilibrium constant to verify the solution.
**Note:** The reaction is exothermic, indicated by the negative enthalpy change (\(\Delta H_{rxn}\)). This might influence the temperature effect on the equilibrium position.
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