i need 2,3,4,5,and 6. 2. (6 Pts) Write the equilibrium expression, Kp, for the reactions in...
All work and answers should be written on your own paper. 1. (6 Pts) Write the equilibrium expression, Kc, for the following reactions. a. 2 SO2(g) + O2(g) = 2 SO3(g) b. Cl(g) + O3(g) = CIO(g) + O2(g) c. 4 KO2() + 2 H2O(g) = 4 KOH(s) + 3 O2(g) 2. (6 Pts) Write the equilibrium expression, Kr, for the reactions in problem 1. 3. (8 Pts) At 127°C, Kc = 2.6 x 10- for the reaction: 2 NH3(g)...
3. (8 Pts) At 127°C, Kc = 2.6 x 10- for the reaction: 2 NH3(g) + N2(g) + 3 H2(g) Calculate Kp at this temperature. 4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gascous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant,...
4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO, and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, Kc. 5. (12 Pts) At a particular temperature, Kc = 1.00 x 10 for the reaction H2(g) + 12(g) = 2 HI(g) In an experiment,...
2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = Kc[RT]An R = 0.08206 L-atm/mol K
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at 625 oC What is Kc at this temperature? Kp = Kc[RT]Δn R = 0.08206 L-atm/mol K
1- The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) --------> H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.395 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M 2- student ran the following reaction in the laboratory at 1090 K: 2SO3(g) ----------> 2SO2(g) + O2(g) When he introduced SO3(g) at a pressure of 1.05 atm into a 1.00...
Be sure to answer all parts. A) Calculate Kp for the following equilibrium: 3 O2(g) ⇌ 2 O3(g) Kc =1.8 × 10 −56 at 450 K __× 10__ B) Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0233 M, [N2] = 0.119 M, and [H2] = 0.369 M. Calculate Kc for the reaction at this temperature. Kc = __
Please answer all six thanks 1) The equilibrium constant for the following reaction is 2.90×10-2 at 1.15×103K. 2SO3(g) ------------------->2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 17.3 L container at 1.15×103K contains 0.437 mol of SO3(g) and 0.422 mol of SO2, the equilibrium concentration of O2 is M. 2) A student ran the following reaction in the laboratory at 1100 K: 2SO3(g) -------------------->2SO2(g) + O2(g) When she introduced 7.74×10-2 moles of SO3(g) into a 1.00 liter...
How many of the following reactions will Kc = Kp? • H2(g) + 12(g) = 2 HI(g) 12(g) + Br2(g) = 2 IBr(g) • SO3(g) + NO(g) =SO2(g) + NO2(g) • 2 HgO(s) = Hg(1) + O2(g) • H2(g) + Br2(g) = 2 HBr(g) • C(s) + O2(g) = CO2(g) 2008 :::
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =