Now let's say that the atmospheric concentration of CO2 has increased to 620 ppm. Calculate the new molar concentration of CO2 in aqueous solution (i. e. in the water sample) once equilibrium is achieved between the 620 ppm CO2 atmosphere and the water sample.
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Now let's say that the atmospheric concentration of CO2 has increased to 620 ppm. Calculate the new molar concentration of CO2 in aqueous solution (i. e. in the water sample) once equilibrium is achieved between the 620 ppm CO2 atmosphere and the water sample.
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- 1. Suppose 1.000 mol CO and 3.000 mol H2 are put in a 10.00 L vessel at 1200 K. The equilibrium constant for Kc for CO(g) + 3H2(g) CH4(g) + H2O(g)equals 3.92. Find the equilibrium composition of the reaction mixture. 2. Boric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solution of boric acid? What is the degree of ionisation of boric acid in this solution? The hydrogen ion arises principally from the reaction:B(OH)3(aq) + H2O(l) B(OH)4(aq)_+ H+(aq)The equilibrium constant for this reaction is 5.9 x 10-10. 3. Calculate the pH of a solution obtained by mixing 500.0 mL of 0.10 M NH3 with 200.0 mL of 0.15 M HCl.Calculate the masses of oxygen and nitrogen that are dissolved in 1.5 L of aqueous solution in equilibrium with air at 25 °C and 760 Torr. Assume that air is 21% oxygen and 78% nitrogen by volume. (See attached picture).22. Write equilibrium constant expressions, in terms of reactant and product concentrations, for each of these reactions. H,O(() H (aq) + OH (aq) CH,COOH(aq) N;(g) + 3 H,(g)=2 NH,(g) K = 1.0 x 10- K = 1.8 x 10 K, = 3.5 x 10 eCH,CO0 (aq) + H* (aq)
- At 25 C, the partial pressure of CO2(g) in a bottle of soda water is 2.9 bar. Calculate the equilibrium concentration of dissolved carbon dioxide under these conditions. The equilibrium constant for dissolving CO2 in water is K = 0.0338Consider the following reactions: CO (g) + 2 H2S (g) D CS2 (g) + H2O (g) + H2 (g) K1 = 1.3 x 105 ½ CH4 (g) + H2S (g) D ½ CS2 (g) + 2 H2 (g) K2 = 180 1. Find the equilibrium constant for: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) 2. What molecules in the steps are reaction intermediates? 3. If 0.500 atm of CO, H2, CH4, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.The equation represents the decomposition of a generic diatomic element in its standard state. X,(g) X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 6.01 kJ-mol at 2000. K and -60.29 kJ-mol- at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. K at 2000. K = K at 3000. K: Assuming that AHixn is independent of temperature, determine the value of AHin from this data. AHixn kJ-mol- %3D Question Source: MRG - General Chemistry F about us privacy policy terms of use contact us help careers
- 22. In a saturated solution of MgF2 at 18°C, the concentration of Mg2* is 2.10 X 103 M. The equilibrium is represented by the following equation: MGF2S) = Mg?* + 2F (aq). Write the expression for the solubility-product constant, Kgp, and calculate its value at 18°C. Note: Show all calculations, follow the rules of significant figures, and box your final answer.The reaction N2O4−⇀↽−2NO2 is allowed to reach equilibrium in a chloroform solution at 25 ∘C . The equilibrium concentrations are 0.327 mol/L N2O4 and 1.91 mol/L NO2 . Calculate the equilibrium constant, Kc , for this reaction. Kc= 11.16 An additional 1.00 mol NO2 is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added. towards the product towards the reactant no change Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc . Kc will increase Kc will not change Kc will decrease Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution. [N2O4]= mol/L [NO2]= mol/L2. Solution is exposed to a partial pressure of NH3 (PNH3 = 5 × 10-9 atm). a. Write down all the equilibrium reactions. b. Define/write down K (or log K) values for the above equilibrium reactions in terms of the relevant concentrations. C. Construct a Tableau for an NH3 gas in an open system with partial pressure. Log K (25 °C) OH-1 -14 NH3 (aq) 1.75 NH4+ -11.05
- Consider the reaction 3A(g)+2B(g)=2C(g)+1D(aq). In 3.1L, 2.79mol A and 2.72mol B are mixed. At equilibrium, 0.573mol D are detected. What is the concentration equilibrium constant (K) of the reaction? Enter your answer to four decimal places if it is less than 1, otherwise answer with a minimum of four digits (ie: 2543, 153.4, 12.52, or 6.523). If your last digit is a trailing zero remember that it's okay that canvas removes it. If it is smaller than 0.0001, enter "0" and make sure you indicate your actual answer clearly on your work.Write the equilibrium expression for the reaction CO (g) + 3 H2 (g) CH4 (g) + H2O (g).A gas-phase reaction mixture contains phosphorus pentachloride, PCI5, phosphorus trichloride, PCI3, and chlorine, Cl2 . At equilibrium, the partial pressures of the gases are 54 kPa, 21 Pa, and 78 Pa, respectively, at 298 K. Calculate the equilibrium constant, K, for the reaction PCI3(g) + Cl2(g) ⇌ PCI5(g) at th is temperature.