3) Equilibrium Conditions 14 Points A 10.0-g sample of solid NH Cl is heated in an...
NH,(8) + HCl(g) NH,Cl(s) A 6.55 g sample of NH, gas and a 6.55 g sample of HCl gas are mixed in a 1.50 L flask at 25°C. Identify the limiting reagent. HCI ONH,CI Ο ΝΗ, How many grams of NH CI will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH, CI produced by the reaction.
When heated, colorless dinitrogen tetraoxide, N2O4(g), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204 (g) + 2 NO2 (g) Suppose that 2.00 mol of N204(g) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K, for this reaction at 407 K. 3.80 2.00 0.500 0.263 0.525
When heated, colorless dinitrogen tetraoxide, N204(8), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204(g) 42 NO2 (g) Suppose that 2.00 mol of N204(8) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K., for this reaction at 407 K. 0.500 O 0.525 2.00 0.263 3.80
PCl_5 decomposes according to the equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) At 700 K, a 2 liter flask initially contained only 0.4600 mol PCl_3(g) and 0.6875 mol PCl_5(g). After reaching equilibrium, 0.00800 mol Cl_2(g) was measured in the flask. Calculate the equilibrium concentrations of the three gases and K_c for the reaction. For the reaction, 2 H_2S(g) 2 H_2(g) + S_2 (g), K_0 = 1.7 times 10^-7 at 800.0 degree C If the initial concentration of H_2S in a closed...
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...
A 10.0 g sample of NH4Cl(s) is heated in an initially evacuated 5.00 L flask to 900 C. The solid ammonium chloride dissociates into NH3(g) and HCl(g) as products; reaction has Kp= 1.44 at this temperature. A). Calculate the partial pressures of NH3(g) and HCl(g) present at equilibrium. B). Calculate the number of moles of NH3(g) and HCl(g) that will be present in the flask at equilibrium. You may neglect the volume of the solid and assume V=5.00 L.
calculate the concentration of PCl5 (g) and PCl 3 (g) at
equilibrium.
Phosphorus pentachloride decomposes according to the chemical equation PCI,() PCI,() + C(®) 1.80 at 250 °C K A 0.131 mol sample of PCI,(g) is injected into an empty 2.05 L reaction vessel held at 250 'C Calculate the concentrations of PCI,(g) and PCI,(g) at equilibrium. M PCI,I Mi PCI,J
Phosphorus pentachloride decomposes according to the chemical equation PCI,(g) = PCI,(8) + Cl (8) K = 1.80 at 250 °C A 0.4421 mol sample of PCI; (g) is injected into an empty 4.60 L reaction vessel held at 250 °C. Calculate the concentrations of PCI;(8) and PCI, (g) at equilibrium. [PCI) = M (PCI,) = M
IEM122_02 Consider the equilibrium A(aq) + B(aq) = C(aq), K = 17.06. A reaction is started with C being the only chemical present and [C, = 0.3825. Compute the B concentration in equilibrium. At 590 °C, the K, for the reaction Caco (s) =Ca0(s) + co (9) expressed in atm is 2.559. A111 gram sample of Caco, is put into a 10.0-L container and heated to 590 °C. Compute the moles co, present in equilibrium. [Hint: R = 0.082057 atm...
CaCO3(s) = Cao (s)+CO2 (g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0 mol sample of CaCO3(s) is placed in a rigid 100. L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00 atm, while some CaCO3(s) remains in the vessel. a. Calculate...