(a) What is the equilibrium constant for the following reaction?
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Physical Chemistry
- When carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)arrow_forwardCalculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.arrow_forwardWrite the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCN (aq) + OH" (aq) CN" (aq) + H,0 (1) K =arrow_forward
- Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2(aq) + H,O(1)=H30*(aq) + NO2 (aq)arrow_forwardCalcium hydroxide will precipitate from solution by the following equilibrium: 2+ Ca²+ (aq) + 2OH(aq) + Ca(OH)₂ (s) Write the equilibrium expression for this reaction.arrow_forwardThe equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.arrow_forward
- Given that K = 2.9 x 109 for the following reaction, Zn2+(aq) + 4 NH3(aq) ⇆ Zn(NH3)42+(aq) what is the value of the equilibrium constant for the reverse reaction?arrow_forwardHere are the equilibrium constants for two reactions of nitrogen with oxygen. What is the equilibrium constant for N₂O (g) + 1/2O₂(g) → 2NO (g)? N₂(g) + O₂(g) = 2NO(g) K= 4.1 × 10^-31 N₂(g) + 1/2O₂(g) = N₂O(g) K=2.4 × 10^-18arrow_forwardWrite the equilibrium constant expression for this reaction: 2 CH;COO (aq)+C,H,O,(aq) → C,H1004(aq)+2 OH (aq)arrow_forward
- 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.arrow_forwardThe equilibrium constant, Kp, for the following reaction is 0.497 at 500 K. Calculate Ke for this reaction at this temperature. C PC15 (g) → PC13(g) + Cl₂ (9) Kc = ||arrow_forwardThe equilibrium constant (KP) for the reaction is 4.24 at 800 K. (a) Calculate AG° for the reaction. (b) Calculate AG for the reaction when the partial pressures are PH2=0.125 atm, PCO2=0.39 atm, PH2O=0.33 atm, and PCO=0.60 atm. 2.arrow_forward
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