Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M) [XY] 0.500 Part B initial: change: equilibrium: 0.100 +x 0.100+ The change in concentration, , is negative for the reactants because they are consumed and positive for the products because they are produced. -H 0.500-2 net → [X] 0.100 +x 0.100 + T 15. ΑΣΦ [XY], [X], [Y] = 0.26,0.34,0.34 + [Y] Based on a K, value of 0.220 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively? Express the molar concentrations numerically. ▸ View Available Hint(s) M

Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M) [XY] 0.500 Part B initial: change: equilibrium: 0.100 +x 0.100+ The change in concentration, , is negative for the reactants because they are consumed and positive for the products because they are produced. -H 0.500-2 net → [X] 0.100 +x 0.100 + T 15. ΑΣΦ [XY], [X], [Y] = 0.26,0.34,0.34 + [Y] Based on a K, value of 0.220 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively? Express the molar concentrations numerically. ▸ View Available Hint(s) M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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2. Please don't write on a paper. I can't understand handwritten.
For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
= KINETICS AND EQUILIBRIUM Setting up a reaction table Suppose a 500. mL flask is filled with 1.7 mol of N₂ and 0.10 mol of NH3. This reaction becomes possible: N₂(g) + 3H₂(g)2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N₂. You can leave out the M symbol for molarity. initial change equilibrium N₂ 0 0 H₂ 0 0 0 NH3 0 0 00 1/5 X
5. Phosphorus pentachloride gas, PCI,(g), will decompose to phosphorous trichloride, PCI,(g), and chlorine, Cl,(g), at 160 °C. In a sealed vessel, the reaction will proceed to equilibrium: PCI,(g) PCI, (g) + Cl(g) A chemist places 3.00 mol of phosphorous penta- chloride gas into a sealed 1.50 L flask at 160 °C. At equilibrium, he observes there is 0.300 mol of phosphorous trichloride gas and some chlorine gas. Calculate the equilibrium concentrations of gaseous phosphorous pentachloride and chlorine. m
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An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) ⇒ CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂ I mol
Part A It is possible to predict the equilibrium constant of a reaction by combining two or more reactions for which the value of K is known. When combining equilibrium constants, it is important to note the following: Determine the value of the equilibrium constant, Kpal, for the reaction • When a reaction is reversed, its K value is inverted; that is, Kreverse = 1/Kforward- • When the coefficients of a reaction are multiplied by a factor, the K value is raised to the power of that factor. • When reactions are added, their K values are multiplied. CO2 (g) = C(s) + 02(g). Kgoal =? by making use of the following information: 1. 2CO2 (g) + 2H20(1) = CH3COOH(1) + 202(g). K1 = 5.40 x 10-16 2. 2H2(g) + O2(g) = 2H,O(1). K2 = 1.06 x 1010 3. CH3COOH(1) = 2C(s) + 2H2(g) + O2(g). K3 = 2.68 x 10 9 Express your answer numerically. • View Available Hint(s) V ΑΣφ Kgoal = Submit Part B Determine the equilibrium constant, Kroal, for the reaction 4PCI, (g) = P4(s) + 10Cl2 (g), Kgoal =? by making use of…
5. The equilibrium constant expression of a gas reaction is [CS2] [H2]* _ [CH4] [H2S]? K. Write the balanced chemical equation corresponding to this expression
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KINETICS AND EQUILIBRIUM Using an equilibrium constant to predict the direction of... A chemical engineer is studying the following reaction: 4 HC1(g) + O₂(g) → 2 H₂O(g) + 2Cl₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.31. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound HC1 0₂ H₂O Cl₂ HCI 0₂ H₂O Cl₂ HCI 0₂ H₂O C1₂ pressure 5.09 atm 5.63 atm 3.31 atm 4.48 atm 3.91 atm 5.34 atm 3.90 atm 5.07 atm 2.74 atm 5.05 atm 4.48 atm 5.65 atm expected change in pressure O ↑ increase ↑ increase O ↑ increase O ↑ increase O ↑ increase ↑ increase ↑ increase O ↑ increase ↑ increase O ↑ increase ↑ increase ↑…
What approximation can be made when the equilibrium constant is very small in order to simplify the math involved with an equilibrium problem? O a) Assume the concentration of each product equals zero. b) Assume this problem cannot be solved by mere humans. c) Assume the reactant concentrations go to zero. d) Assume that the reactant concentrations do not change significantly.
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