4. Open bodies of water can act as carbon sinks due to the ability of carbon dioxide to dissolve in water. The dissolution of carbon dioxide produces carbonic acid (H₂CO3) which then partially dissociates in an equilibrium reaction important for controlling water pH. CO₂ (g) + H₂O (1)→ H₂CO3(aq) H₂CO3 (aq) H+ (aq) + HCO3 (aq) The equilibrium between carbonic acid (H₂CO3) and bicarbonate (HCO3) is influenced by the presence of dissolved metals from the bedrock underlying a body of water. Calcium from limestone (a type of sedimentary rock formed from marine exoskeletons) is one such metal. The graph below shows how the concentration of dissolved calcium ions (measured in parts per million, or mg/L) affects the concentration of carbon dioxide dissolved in ocean water (measured partial pressure). Based on this graph and your understanding of equilibrium, in what direction does the presence of limestone shift the carbonic equilibrium? acid/bicarbonate 10-4 10-3 Closed Calcite saturation- Closed Open 10-² CO₂ pressure (atm) Open 10-1 400 T 300 200 1 100 Ca2+ concentration (ppm) (0.463) to noutaks

4. Open bodies of water can act as carbon sinks due to the ability of carbon dioxide to dissolve in water. The dissolution of carbon dioxide produces carbonic acid (H₂CO3) which then partially dissociates in an equilibrium reaction important for controlling water pH. CO₂ (g) + H₂O (1)→ H₂CO3(aq) H₂CO3 (aq) H+ (aq) + HCO3 (aq) The equilibrium between carbonic acid (H₂CO3) and bicarbonate (HCO3) is influenced by the presence of dissolved metals from the bedrock underlying a body of water. Calcium from limestone (a type of sedimentary rock formed from marine exoskeletons) is one such metal. The graph below shows how the concentration of dissolved calcium ions (measured in parts per million, or mg/L) affects the concentration of carbon dioxide dissolved in ocean water (measured partial pressure). Based on this graph and your understanding of equilibrium, in what direction does the presence of limestone shift the carbonic equilibrium? acid/bicarbonate 10-4 10-3 Closed Calcite saturation- Closed Open 10-² CO₂ pressure (atm) Open 10-1 400 T 300 200 1 100 Ca2+ concentration (ppm) (0.463) to noutaks

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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Gypsum (CaSO4·2H2O) is added to soil to enhance plant growth. It dissolves according to the following equation: CaSO4⋅2H2O(s)⇌Ca2+(aq)+SO2−4(aq)+2H2O(1)CaSO4⋅2H2O(s)⇌Ca2+(aq)+SO42−(aq)+2H2O(1) The Ksp of gypsum is 3.14 × 10−5. How much gypsum, in grams, should you add to your 5.0 L watering can to produce a saturated solution?
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.
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Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.2 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.5 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = ☐ x10 ×
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