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A mixture containing 3.9 moles of NO and 0.88 mole of CO2 was allowed to react in a flask at a certain temperature according to the equation: NO(g)+CO2(g)NO2(g)+CO(g) At equilibrium, 0.11 mole of CO2 was present. Calculate the equilibrium constant Kc of this reaction.

Short Answer

Expert verified
The equilibrium constant, Kc, is 1.722.

Step by step solution

01

Write the balanced equation and define changes

The balanced equation for the reaction is NO(g)+CO2(g)NO2(g)+CO(g). Initially, we have 3.9 moles of NO and 0.88 moles of CO2. If x moles react, the change in moles will be: x for both NO and CO2, and +x for both NO2 and CO.
02

Determine the equilibrium moles

At equilibrium, the number of moles of CO2 is given as 0.11 moles. Therefore, 0.88x=0.11, solving this gives x=0.77. Thus, the equilibrium moles are: NO=3.90.77=3.13, CO2=0.11, NO2=0.77, and CO=0.77.
03

Calculate equilibrium concentrations

To find the concentration, assume the reaction occurs in a 1 L flask, hence moles equal concentrations (Molarity), giving: [NO]=3.13, [CO2]=0.11, [NO2]=0.77, and [CO]=0.77.
04

Write the equilibrium expression

The equilibrium constant expression is Kc=[NO2][CO][NO][CO2]. Insert the equilibrium concentrations into this equation.
05

Calculate the equilibrium constant

Substitute the values into the expression to find Kc: Kc=(0.77)(0.77)(3.13)(0.11)Calculate to get:Kc=0.59290.3443=1.722

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Equilibrium
Chemical equilibrium is a state in which the rates of the forward and reverse reactions are equal in a chemical reaction. This means there's no net change in the concentrations of reactants and products over time. In our example, the reaction between nitric oxide (NO) and carbon dioxide (CO2) forms nitrogen dioxide (NO2) and carbon monoxide (CO).
Equilibrium signifies balance in the reaction process. Although the amounts of NO, CO2, NO2, and CO don't change at equilibrium, the chemicals continue to react. This continuous reaction is called dynamic equilibrium.
Understanding chemical equilibrium is crucial because it determines the concentrations of reactants and products, leading to the calculation of the equilibrium constant, Kc. This constant helps predict the extent of the reaction and the potential yield of products.
Reaction Stoichiometry
In the world of chemistry, stoichiometry refers to the quantitative relationship between elements in a chemical reaction. The balanced equation for a chemical reaction provides this stoichiometric relationship and allows chemists to predict the amounts of substances consumed and produced.
In our balanced reaction NO(g)+CO2(g)NO2(g)+CO(g), each molecule of NO reacts with one molecule of CO2 to produce one molecule each of NO2 and CO. This is a 1:1:1:1 stoichiometric relationship.
Stoichiometry helps in calculating the changes in the number of moles of each substance as the reaction proceeds toward equilibrium, which further aids in determining the equilibrium concentrations.
Balanced Equation
A balanced chemical equation is essential for understanding the chemical reaction's stoichiometry. It represents the number of units of each reactant and product involved in the reaction.
For our example, the balanced equation is: - NO(g)+CO2(g)NO2(g)+CO(g).
This equation showcases the law of conservation of mass, where the number of atoms for each element is the same on both sides of the equation. Balancing ensures that the reaction accurately represents the real-life process.
With the equation properly balanced, it's possible to track how the number of molecules changes as the reaction progresses, directly impacting the calculation of the equilibrium state.
Concentration Calculation
Calculating concentrations is a critical step in understanding chemical reactions at equilibrium. Concentration is measured in Molarity, M, which is moles per liter. In equilibrium calculations, knowing the volume of the reaction mixture is crucial.
In our exercise, we assume the reaction occurs in a 1 L flask, which makes moles equal concentrations. Thus, the equilibrium concentrations of the substances become directly related to their moles:
  • [NO]=3.13
  • [CO2]=0.11
  • [NO2]=0.77
  • [CO]=0.77
These concentrations allow the calculation of the equilibrium constant Kc, providing insights into the reaction's behavior and directionality. Using such calculations sets the foundation for predicting product yields and optimizing conditions for chemical processes.

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Most popular questions from this chapter

The equilibrium constant KP for the reaction: 2H2O(g)2H2(g)+O2(g) the same temperature? (b) The very small value of KP (and Kc ) indicates that the reaction overwhelmingly favors the formation of water molecules. Explain why, despite this fact, a mixture of hydrogen and oxygen gases can be kept at room temperature without any change.

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