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2. Using the equilibrium constant expressions, you determined on # 1, calculate the value of K when: a. [N₂] = 0.0100 M, [H₂] = 0.0200 M, [NH3] = 0.0300 M b. [H₂O] 3.0 M, [H₂] = 0.0200 M c. [0₂] = 0.0100 M d. [H] = 1 x 105 M, [OH-] = 1 x 10³ M e. [CO₂] = 5.0 M, [O₂] = 2.0 M, [CO] = 3.0 M

2. Using the equilibrium constant expressions, you determined on # 1, calculate the value of K when: a. [N₂] = 0.0100 M, [H₂] = 0.0200 M, [NH3] = 0.0300 M b. [H₂O] 3.0 M, [H₂] = 0.0200 M c. [0₂] = 0.0100 M d. [H] = 1 x 105 M, [OH-] = 1 x 10³ M e. [CO₂] = 5.0 M, [O₂] = 2.0 M, [CO] = 3.0 M

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
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. Using the equilibrium constant expressions, you determined on # 1, calculate the value of K when: a. [N₂] = 0.0100 M, [H₂] = 0.0200 M, [NH3] = 0.0300 M b. [H₂O] 3.0 M, [H₂] = 0.0200 M c. [0₂] = 0.0100 M d. [H] = 1 x 105 M, [OH-] = 1 x 10³ M e. [CO₂] = 5.0 M, [O₂] = 2.0 M, [CO] = 3.0 M
Transcribed Image Text:2. Using the equilibrium constant expressions, you determined on # 1, calculate the value of K when: a. [N₂] = 0.0100 M, [H₂] = 0.0200 M, [NH3] = 0.0300 M b. [H₂O] 3.0 M, [H₂] = 0.0200 M c. [0₂] = 0.0100 M d. [H] = 1 x 105 M, [OH-] = 1 x 10³ M e. [CO₂] = 5.0 M, [O₂] = 2.0 M, [CO] = 3.0 M
a. N₂ (g) + 3 H₂ (g) = 2 NH3 (9) b. 3 Fe (s) + 4 H₂O (g) Fe3O4 (S) + 4 H₂ (9) c. 2 KCIO3 (S) 2 KCI (s) + 3 O2 (g) d. H₂O (1) H* (aq) + OH- (aq) e. 2 CO (g) + O2 (g) = 2 CO₂ (g) f. Li₂CO3 (S) = 2 Li + (aq) + CO3² (aq)
Transcribed Image Text:a. N₂ (g) + 3 H₂ (g) = 2 NH3 (9) b. 3 Fe (s) + 4 H₂O (g) Fe3O4 (S) + 4 H₂ (9) c. 2 KCIO3 (S) 2 KCI (s) + 3 O2 (g) d. H₂O (1) H* (aq) + OH- (aq) e. 2 CO (g) + O2 (g) = 2 CO₂ (g) f. Li₂CO3 (S) = 2 Li + (aq) + CO3² (aq)
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