Ammonia reacts slowly in air to produce nitrogen monoxide and water vapor: NH 3 (g) + O 2 (g) ⇌ NO(g) + H 2 O(g) + Heat b. Write the equilibrium equation.

Hello. In this problem, we're told phosphorous chloride is formed by the reaction of phosphorous tri chloride with oxygen. Were asked to provide the equilibrium expression. To begin. We need to balance our reaction. We have phosphorous tri chloride reacting with oxygen gas form phosphorous chloride. As it's written, the phosphorus and chlorine a balance. But the oxygen is not, you can begin by putting a coefficient of one half out in front of the oxygen. We now have one oxygen on both sides. We don't want to keep the fraction. So we'll multiply through by two, we then get two moles of phosphorus chloride Reacting with one mole of oxygen gas To give us two moles of phosphorus chloride. Writing our equilibrium constant expression. We have our product concentration to the phosphorous chloride which is raised to the coefficient in the balanced reaction equation, which is two. So we'll square that divided by the concentration of phosphorus tri chloride. The coefficient is two. So we'll square the concentration and then we have the concentration of oxygen. And the coefficient is one, we look at the answers that are provided, we see that a then matches the equilibrium constant expression that we wrote. So the correct answer then is a thanks for watching. Hope this helped.

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7. Energy, Rate and Equilibrium

The Equilibrium Constant

GOB Chemistry

7. Energy, Rate and Equilibrium

The Equilibrium Constant

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Problem 73b

Textbook Question

Ammonia reacts slowly in air to produce nitrogen monoxide and water vapor:
NH₃(g) + O₂(g) ⇌ NO(g) + H₂O(g) + Heat
b. Write the equilibrium equation.

Verified step by step guidance

Step 1: Begin by writing the balanced chemical equation for the reaction. The given reaction is NH₃(g) + O₂(g) ⇌ NO(g) + H₂O(g) + Heat. To balance it, ensure that the number of atoms of each element is the same on both sides of the equation.

Step 2: Balance the nitrogen (N) atoms. There is 1 nitrogen atom in NH₃ on the reactant side and 1 nitrogen atom in NO on the product side. This is already balanced.

Step 3: Balance the hydrogen (H) atoms. There are 3 hydrogen atoms in NH₃ on the reactant side. On the product side, H₂O contains 2 hydrogen atoms. To balance, place a coefficient of 2 in front of NH₃ and a coefficient of 3 in front of H₂O.

Step 4: Balance the oxygen (O) atoms. On the reactant side, O₂ contains 2 oxygen atoms. On the product side, NO and H₂O contribute oxygen atoms. Adjust the coefficients to balance the oxygen atoms.

Step 5: Verify that all elements are balanced and write the final equilibrium equation. Ensure that the reaction is reversible (indicated by the ⇌ symbol) and includes the heat term to indicate that it is exothermic.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the context of the given reaction, this means that ammonia (NH3) and oxygen (O2) are converting to nitrogen monoxide (NO) and water vapor (H2O) at a rate that balances with the reverse process, allowing the system to maintain a stable state.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, each raised to the power of their coefficients in the balanced equation. For the reaction provided, K can be calculated using the concentrations of NO and H2O divided by those of NH3 and O2, reflecting the extent to which the reaction favors products or reactants.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle is crucial for understanding how changes in concentration, temperature, or pressure can affect the position of the equilibrium in the reaction between ammonia and oxygen.