Explain the chemistry behind ocean acidification. You should include the formation of carbonic acid from carbon dioxide, how this reacts with carbonate ions, and how continued CO2 emission will impact ocean pH.

In sediments and waterlogged soil, dissolved O2 concentrations are so low that the microorganisms living there must rely on other sources of oxygen for respiration. Some bacteria can extract the oxygen in sulfate ions, reducing the sulfur in them to hydrogen sulfide gas and giving the sediments or soil a distinctive rotten-egg odor.Write the net ionic equation for the reaction under acidic conditions (H3O+) that releases O2 from sulfate and forms hydrogen sulfide gas. Use water as the reactant in the half-reaction that describes the formation of oxygen.

Hydrogen, a potential fuel, is found in great abundance in water. To separate the hydrogen from the oxygen, water must be thermally decomposed. At 1000°C, the equilibrium constant for this reaction is 7.3 x 10-182H2O(g) + heat <-> 2H2(g) + O2(g) a) If the initial concentration of H2O is 0.350 M, what is the equilibrium concentration of H2? b) Suggest three stresses that could be applied to the equilibrium system to produce more hydrogen.

Predict the equilibrium concentration of NH in the reaction described below (for which Kc = 1.210 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. = NHSH(s) NH¸(g) + H₂S(g) Using the data from your ICE Table (Part 1), construct the expression for the equilibrium constant, Kc. Each reaction participant must be represented by one tile. Do not combine terms. KC = II = 1.2 × 10-4 RESET [x] [2x] [2x]² [1.2 × 104+x] [1.2 × 104-x] [1.2 × 104 + 2x] [1.2 × 104 -2x] [1.2 × 10+ + x]² [1.2 × 10+ - x]² [1.2 × 10+ + 2x]² [1.2 × 104 -2x]²

Answer the following

Consider the reaction: N2(g) + 3H2(g) 2NH3(g) where Kc = 0.500 at 400 °C. If 50.0 L reaction vessel contains 1.000 mole N₂; 3.000 mole H₂ and 0.050 mole NH3, which of the following is TRUE? The reaction based on the following parameters is in equilibrium. More ammonia will be produced as the reaction approaches equilibrium. Data provided is not enough to warrant a conclusion regarding equilibrium. More ammonia will dissociate as the reaction approaches equilibrium.

The reaction 2CO(g) + O2(g) = 2 CO2(g) is known to be exothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.

Most reaction do not go to completions. Equilibrium is established between the reactants and products. For the reaction of A with B to produce C and D, we can write the chemical equation as: аА + bв + сс + dD where + represents equilibrium between the reactants and products. The extent to which the reaction proceeds to product formation, at a given temperature, is given by the equilibrium constant, Kę. The equilibrium constant is written mathematically (for the above equation) as: [C[[D]* K. = [A]°[B]" where, a, b, c, and d are the stoichiometric coefficients from the balanced chemical equation and the brackets, [ ], indicate molar concentration. 1. For the following reaction: 2A + В + 3с calculate the equilibrium constant, K, if at equilibrium the concentration of A is 0.15M, the concentration of B is 0.20M, and the concentration of C is 0.10M.

Write the pressure equilibrium constant expression for this reaction. 2 CO,(g)+4 H,O(g)→2CH;OH(1)+3 O2(9)

What are the pH and pOH of 0.075 M NaOH(aq)?