I know how to solve it but want to make sure i did it right thx ### Calculating Equilibrium Composition from an Equilibrium Constant#### Problem Statement:Suppose a 500. mL flask is filled with 1.2 mol of CO, 0.20 mol of H₂O, and 0.30 mol of CO₂. The following reaction becomes possible:\[ \text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g) \]The equilibrium constant \( K \) for this reaction is 3.07 at the temperature of the flask.Calculate the equilibrium molarity of \( \text{H}_2\text{O} \). Round your answer to two decimal places.#### Input Area:An input box is provided for students to enter the molarity, denoted as \( \boxed{M} \).#### Additional Features:1. **Calculation Buttons:** - \( \boxed{\times} \): Likely used for deleting an entry. - \( \boxed{\curvearrowright} \): Likely used for reloading or refreshing the input. - \( \boxed{?} \): Likely used for accessing help or hints.2. **Explanation Button:** - A button labeled "Explanation" where students can get a detailed solution.3. **Check Button:** - A button labeled "Check" to verify the entered answer.#### Diagram Description:No specific diagrams provided, but the problem requires understanding of chemical equilibrium and molarity calculations.**Source:**© 2022 McGraw Hill LLC. All Rights Reserved. **Navigation:**This task is part of an online educational platform, featuring a step-by-step progress bar indicating completion status, and several navigation buttons for additional learning support and tools.### Educational Objectives:- Understand and apply the concept of equilibrium constant.- Perform molarity calculations to find the equilibrium concentrations.- Engage with interactive tools for enhanced learning and immediate feedback.

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Suppose a 500. mL flask is filled with 1.2 mol of CO, 0.20 mol of H₂O and 0.30 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 3.07 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X

Suppose a 500. mL flask is filled with 1.2 mol of CO, 0.20 mol of H₂O and 0.30 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 3.07 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.40PAE: Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that...

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The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Consider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?
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A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
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