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(e) In the following empty box, draw an appropriate number of each type of molecule to represent a possible new equilibrium at the lower temperature. • H2 12 IH O

(e) In the following empty box, draw an appropriate number of each type of molecule to represent a possible new equilibrium at the lower temperature. • H2 12 IH O

Chemistry
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
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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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(e) In the following empty box, draw an appropriate number of each type of molecule to represent a possible new equilibrium at the lower temperature. • H2 IH O
Transcribed Image Text:(e) In the following empty box, draw an appropriate number of each type of molecule to represent a possible new equilibrium at the lower temperature. • H2 IH O
Question #2: For parts of the question that require calculations, clearly show the method used and the steps involved in arriving at your answers. Examples and equations may be included in your answers where appropriate. Gas Initial Concentration (M) H3 0.030 0.015 HI Samples of three gases, H,(g), L(g), and HI(g), were combined in a rigid vessel. The initial concentrations of H,(g) and L(g) are given in the table above. (a) The original value of the reaction quotient, Q, for the reaction of H,(g) and L(g) to form HI(g) (before any reaction takes place and before equilibrium is established), was 5.56. On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas. 0.080 0.070 0.060 0.050 0.040 0.030 0.020 0.010 0.000 Time Equilibrium was established at a certain temperature according to the following chemical equation. H,(g) + L(g) 2 2HI8) AH°= -9.4 kl/mol: K, = 49 After the equilibrium was established, the concentration of H,(g) was 0.020 M. (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part (a). The curves must show how the concentration of each of the three gases changed as equilibrium was established. H,(g), L(g), and HI(g) are at equilibrium at a different temperature in a different vessel. (c) When the temperature in the vessel is decreased, does the equilibrium shift to the right, favoring the product, or to the left, favoring the reactants? Justify your answer. (d) Does the value of K, increase, decrease, or remain the same when the temperature is decreased? Justify your answer based on the expression foe K, and the concentrations of the product and reactants. Concentration (M)
Transcribed Image Text:Question #2: For parts of the question that require calculations, clearly show the method used and the steps involved in arriving at your answers. Examples and equations may be included in your answers where appropriate. Gas Initial Concentration (M) H3 0.030 0.015 HI Samples of three gases, H,(g), L(g), and HI(g), were combined in a rigid vessel. The initial concentrations of H,(g) and L(g) are given in the table above. (a) The original value of the reaction quotient, Q, for the reaction of H,(g) and L(g) to form HI(g) (before any reaction takes place and before equilibrium is established), was 5.56. On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas. 0.080 0.070 0.060 0.050 0.040 0.030 0.020 0.010 0.000 Time Equilibrium was established at a certain temperature according to the following chemical equation. H,(g) + L(g) 2 2HI8) AH°= -9.4 kl/mol: K, = 49 After the equilibrium was established, the concentration of H,(g) was 0.020 M. (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part (a). The curves must show how the concentration of each of the three gases changed as equilibrium was established. H,(g), L(g), and HI(g) are at equilibrium at a different temperature in a different vessel. (c) When the temperature in the vessel is decreased, does the equilibrium shift to the right, favoring the product, or to the left, favoring the reactants? Justify your answer. (d) Does the value of K, increase, decrease, or remain the same when the temperature is decreased? Justify your answer based on the expression foe K, and the concentrations of the product and reactants. Concentration (M)
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