PCl_5 decomposes according to the equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) At 700 K, a 2...
Phosphorus pentachloride decomposes according to the chemical equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) K_c = 1.80 at 250 degree C 0.239 mol sample of PCl_5(g) is injected into an empty 3.05 L reaction vessel held at 250 degree C. Calculate the concentrations of PCl_5(g) and PCl_3(g) at equilibrium.
Please help Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl_5(g) PCl_3(g) + Cl_2(g) At 250 degree C, 0.250 M PCl_5 is added to a flask. If K_C = 1.80, what are the equilibrium concentrations of each gas? A) [PCl_5] = 2.27 M, [PCl_3] = 2.02 M, [Cl_2] = 2.02 M B) [PCl_5] = 0.0280 M, [PCl_3] = 0.222 M, [Cl_2] = 0.222 M C) [PCl_5] = 1.25 M, [PCl_3] = 0.474 M, [Cl_2] =...
The equilibrium constant, K, for the following reaction is 1.20 times 10^-2 at 500 k. PCl_5 (g) irreversible PCl_3 (g) + Cl_2 (g) At equilibrium mixture of the three gases in a 1.00 L. flask at 500 K contains 0.203 M PCl_5, 4.93 times 10^-2 M PCl_5 and 4.93 times 10^-2 M Cl_2. What will be the concentration of the three gases once equilibrium has been reestablished, if 2.81 times 10^-2 mol of PCl_3 (g) is added to the flask?...
For the reaction PCl_5(g) ⇌ PCl_3(g) + Cl_2(g) at equilibrium, K_p = 321. The equilibrium partial pressures of PCl_3 and Cl_2 are 1.43E0 atm and 4.07E0 atm, respectively. What is the equilibrium partial pressure of PCl_5?
At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of the gases at 1500 K are 0.0064 mol/L for BrF_5, 0.0018 mol/L for Br_2, and 0.0090 mol/L for F_o. Calculate the value of K_r. The reaction of iron and water vapor results in an equilibrium 3Fe(s) + 4H_2O(g) Fe_3O_4(s) + 4H_2(g) and an equilibrium constant, K_c, of 4.6 at 850 degree C. What is the concentration of hydrogen present at equilibrium if the reaction...
An decrease in temperature increases the reaction rate because temperature affects the equilibrium constant of the reaction a smaller fraction of the collisions have the correct orientation of molecules. the activation energy of the reaction will decrease. less collisions will have enough energy to exceed the activation energy. the activation energy of the reaction will increase. The equilibrium constant, K_p, for the reaction H_2(g) + I_2(g) doubleheadarrow 2HI(g) is 10.0 at 450 degree C. A rigid cylinder at that temperature...
The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar concentration for SO_3 is 0.675 M ([SO_3| = 0.675 M) and the initial molar concentration for CO_2 is 0.444 M (|CO_2] = 0.444 M). After the reaction reached equilibrium the concentration of CO_2 now equals 0.214 M ((CO_2] = 0.214 M). What is the K_c value for the reaction? 0.00987 0.0342 7.31 11.8 16.7 At 35 degree C the equilibrium constant value (K_c) for...
The equilibrium constant, K. for the following reaction is 1.20 times 10^2 at 500 K An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.166 M PCl_5 4.47 times 10^-2 MPCl_5 and 4.47 times 10^-2 M Cl_2 What will be the concentrations of the three gases once equilibrium has been re-established if 3.26 times 10^-2 mol of Cl_2(g) is two gases once equilibrium has been reestablished? [NH_3} = M [H_2S] = M
Nitrosyl bromide decomposes according to the following equation 2NOB (g) + 2NO(g) + Bry (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Bry. At equilibrium the flask contained 0.16mol of NOBr. How many moles of NO and Br. respectively, are in the flask at equilibrium? 0.16 0.16 0.24, 0.42 0.48.0.48 0.16, 0.00 0.48.0.24
2. The compound NOCI decomposes to nitric oxide and chlorine according to the following equation: 2 NOCI (g) 2 NO (g+ Cl (g) Suppose that 0.480 mol NOCI is placed in a 5.00-L flask at a given temperature. When equilibrium has been established, is found that the concentration of NO is 0.0196 M. Calculate the equilibrium constant for this reaction.