1. Write the equilibrium constant expressions (both Ke and Kp, where applicable) for the following reactions...
2) Write the equilibrium constant expressions for each of the following reactions. (For gas-phase reactions, write the Ke expression.) a) 2 NO(g) + O2(g) = 2 NO2(g) b) 4 Ag(s) + O2(g) + 2 Ag2O(S) c) CaCO3(s) + CO2(aq) + H2O(l) = Ca2+(aq) + 2 HCO3(aq) 3) a) Write the K, expressions for reactions a and b in problem 2. b) If the value of K for reaction a in problem 2 is 2.8 x 1011 at 200°C, what is...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions: (a) H(g)Cl(g) 2 HCl(g) (b) 2 C(s)+O2(g) 2 CO(g Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 O(g) 3 0:(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O, and 0.060 mol of NO2 at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant Ke for the reaction? N2O4(g) 2 NO:(g)...
Write equilibrium constant expressions, Kp, for the following reactions. i) N2(g) + 3 H2(g) ⇌ 2NH3(g) ii) NH4HS(s) ⇌ NH3(g) + H2S(g)
1. Write down the equilibrium constant expressions, K, and K for each of the following reactions: (a) H2(g)C(g) 2 HCl(g) (b) 2 C(s)+0(g) 2 COg Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 0,(g) 30,(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O and 0.060 mol of NO, at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant K, for the reaction? N,0,(g)2 NO(g) 3. Ammonium...
Review 1: Equilibrium 1. Write equilibrium expressions for the following reversible reactions: a. 2 NO: (g=N.O.( b. N. (g) + 3 H2(g) = 2 NH, (g) c. 2 SO, (g) + O2(g) = 2 SO, (g) 2. For the equilibrium system described by 2 SO2(g) + O(g) = 2 SO, (g), the equilibrio concentrations of SO, O, and SO, were 0.75 M, 0.30 M, and 0.15 M, respectively. Calculate th equilibrium constant, Keq, for the reaction. 3. Keq = 35...
Write the expressions for the equilibrium constants of the following reactions, that includes the mass action relationships (i.e., the ratio of standardized partial pressures) and the value of the equilibrium constant calculated from the Gibbs energies of reaction: a) CO2(g)+Cl2(g) <->COCl(g)+Cl(g) b)2SO2(g)+)O2(g) <-> 2SO3(g) c)H2(g)+Br2(g) <-> 2HBr(g) d)2O3(g) <-> 3O2(g)
For the following equilibrium, CUSO4-5H2O (s) CuSO4 (s) + 5 H20 (g) a) Write the expressions of equilibrium constants, Ke and Kp. b) Use an equation to show the relationship between Ke and Kp.
Worksheet 15a (Intro) Rates & Equilibrium 5. Write the equilibrium expressions K, for each of the following reactions: a. Na(g) + O2(8) 2NO(g) e. PC1:(g) =PC13(1) + Cl () b. SiH.(g) + 2C1_(g) = Siclag) + 2H2(g) f. Xe(g) + 3F5(g)=XeF6Kg) c. C(s) + CO/g) = 2CO(g) g. Pb(NO:) (aq) + 2KI(aq) = Pbl (s) + 2KNO (aq) d. Fe(s) + CO(g) = Fe(s) -CO(8) h. 2NaCl(s) + 302(g) + 2NaClO(s)
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
1. Write equilibrium expressions for each of the following reactions (*Concentration of a solid is a constant) SICL(g) + 2H2 (g) Si(s) +4HCI(g) a. 2+ Zn(s) + Fe Zn (aq) + Fe(s) b. (aq) lculate the value of the equilibrium constant of the reaction of SO, and Wat e H2SO4 when the concentrations at equilibrium are as follows [SO] = 0 -0.480M H,O@ HSO + 40