For the reaction between ethylene and chlorine, the equilibrium constant is 2.00x10^6. If the initial concentrations of ethylene and chlorine are .250 M, what are the equilibrium concentrations of ethylene and chlorine?
C2H4+Cl2-> C2H4Cl2
For the reaction between ethylene and chlorine, the equilibrium constant is 2.00x10^6. If the initial concentrations...
The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362 M, calculate the [Br] =
The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362 M, calculate the [Br] =
The equilibrium constant for the reaction below is Kc=115. if the initial concentrations of F2, H2 and HF are all 2.0 M, what are the equilibrium concentrations of H2 and HF? F2(g) + H2(g) <--> 2HF(g)
Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) ⇌ C2H5OH(g) Kc = 9.0 × 104 [C2H4]eq = 0.95 M [C2H5OH]eq = 5.03 M A. A) 9.9 × 10-7 M B. B) 80.0 M C. C) 5.9 x 10-5 D. D) 1.68 M E. E) 0.021 M F. F) none of these
Calculate the equilibrium concentrations of H2O, Cl, HCl, and O2 at 298 K if the initial concentrations are (H2O) = 0.070 M and (Cl2] = 0.120 M. The equilibrium constant Kc for the reaction H2O(g) + Cl2(g) + 2HCl(g) + O2(g) is 8.96 x 10 -9 at 298 K
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
Consider the following reaction. Initial concentration, and equilibrium constant at a particular temperature. Determine the equilibrium concentrations of SO2. SO,Cl2(g) 5 SO2(g+ + Cl2(g) Kp = 8.99 x 107 [SO_C12] = 0.125M A) 7.19 x 10-6M B) 3.35 x 10 *M C) 2.25 x 10-'M D) 2.68 x 10M E) 1.12 x 10'M
Calculate the equilibrium constant for the hydration reaction of ethylene with water to produce ethanol at a temperature of 280 K and a pressure of .8 atm C2H4(g) + H2O(g) ? C2H5OH(g) ?H?rxn = -47.8 kJ Kc = 9 x 103 at 600K
19) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(8) + H2O(g) - C2H5OH(g) Kc = 9.0 x 103 (C2H4leq=0.015 M [C2H5OHleq=1.69 M A) 1.0 M B) 9.9 x 10-7 M C) 0.013 M D) 1.68 M E) 80.M 20) Consider the following reaction at equilibrium. What effect will increasing the volume of the reactic mixture have on the system? 20) 2 H2S(8) + 3 O2(g) + 2 H2O(g)...
The equilibrium constant, K, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(8) = 2NOCI(g) is 6.5 x 104 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl., and NOCI are 2.6 x 10-3 M, 7.4 x 10-M, and 5.8 M respectively? o o O shift right shift lent neither
Answer the questions about the following reaction below. The equilibrium constant for the decomposition of PCls at 250°C is 0.041 ΔH is positive; reactants and products are gases at 250°C. Refer to your textbook. 1. Is the reaction above exothermic or endothermic? 2. What happens to the concentrations of PCls and Cl if more PCls is added once the reaction reaches equilibrium? (increases, decreases) PC1s Cl2 3. What happens to the moles of PCIs, PCls and Cl in the container...