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alkalinity
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- For the reaction aA(aq) + bB(1) cC(g) + dD(aq) the equilibrium constant, K, can be written as Pc- [D]d [A]a K= The equilibrium constant is unitless because the units always mathematically cancel when the pressure is expressed in torr and concentration is expressed in molality. each quantity is a dimensionless ratio of the actual concentration or pressure divided by standard state concentration or pressure. pressure and concentration are unitless quantities. taking each pressure or concentration to its coefficient power cancels out the units.The dissociation of NH.CI (s) = NH, (g) + HCI (g) at 0.41 bar has a chemical equilibrium, K, of 2.6 x 10. a) Give the expression of K in terms of degree of dissociation, a. ( b) Calculate the value of aA mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. (CH3);CCI(g) = (CH3),CCH2(g) + HCI(g) Based on your ICE table, set up the expression for K for the decomposition of (CH3);CCI. (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 Do not combine or simplify terms. K = 3.45 5 RESET (P(CH);CCH;) (P(CH,);CCH,)? (PHCI) (Рнс) (P(CH,),cCi) (P(CH,),CCI)? 2(Рнс) 2(P(CH3),CCH;) 2(P(CH,),CCI) 2(P(CH,),CCI)? 2(Рнс)? 2(P(CH3),C=CH,)?
- 6B.4(b) The equilibrium constant for the reaction N2(g) + O2(g)=2 NO(g) is 1.69×10-3 at 2300 K. A mixture consisting of 5.0 g of nitrogen and 2.0 g of oxygen in a container of volume 1.0 dm³ is heated to 2300 K and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.20Consider the reaction at 25 degrees celsius 2NO3-(aq)+8H^+(aq)+3Cu(s)=3Cu2+(aq)+2NO(g)+4H2O(l) At what pH is the reaction at equilibrium with all other ionic species at 0.01M and gases at 1 atm?(a) N₂(g) + O₂(g) = 2NO(g) (b) BaSO3(s) BaO(s) + SO₂(g) (c) NH3(aq) + H₂O (1) For the following reactions, write the mathematical expression for the reaction quotient, Qc,: NH4+ (aq) + OH-(aq) (d) Br₂(g) = 2Br(g) (e) 2SO₂(g) + O₂(g) = 2SO3(g) (f) NH₂(g) +20₂(g) = CO₂(g) + 2H₂O(1) 10 (h) N₂(g) + 3H₂(g) = 2NH3(g) (i) NH₂Cl(s) = NH3(g) + HCl(g) (1) CO₂(g) + H₂(g) = CO(g) + H₂O(g) openstax Which systems are homogeneous (heterogeneous) equilibria? acid-base equilibria?
- A mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. bar (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 What is the partial pressure of isobutylene ((CH3)2CCH2) at equilibrium? 4 C 8. 9. +/- х 100A mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. bar (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 You have calculated the equilibrium partial pressures to be: 4 C tert-butyl chloride,CH3);CCI = (x) hydrochloric acid, HCI = (0.600 - x) isobutylene, (CH3)2CCH2 = (0.400 - x) What is the partial pressure of tert- butyl chloride ((CH3)3CCI) at equilibrium? 8. 9. +/- х 100calculate the value of the equilibrium constant, Rc₂ Q (g) + x (g) = 2 M(g) + N(0) given that KC₁ - 3.20 ког = 0.443 14.0 Кез Meg) = 2(g) 6Rcg) = 2 N(g) + 47 (8) 3 X (9) +30)(9) — 9R(g) R= ? GIVE EXPLAINED HANDWRITTEN ANSWER
- Solid NH4I ammonium iodide (which is always considered to be in excess) is introduced into an initially empty container at a constant temperature of 427°C. An equilibrium is quickly established and the total pressure (PT) is then 0.9 bar. NHẠI (s) 2 NH3(g) + HI(g) Express the equilibrium constant K' of this reaction as a function of PT a. Express the equilibrium constant K' of this reaction as a function of PT- The answer is PNH, PHI - - ( 2 2 P K' || po2 p°2 2P°, Can you explain why we get (p/2)^2?For the reaction PCl5(g) <=> PCl3(g) + Cl2(g), the equilibrium constantKc = 1.1 * 10-2 at 400 K. What is the equilibrium constant for the reactionPCl3(g) + Cl2(g) <=> PCl5(g) at 400 K?C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalyst