7 Consider the following reaction at 298 K: NH3(g) +HCI(g)NH4CI(s) Using the thermochemical data at 298 K given below (a) Determine the AH for the reaction. (2 marks) (b) Determine the AG for the...
The equilibrium constant, K, for the following reaction is 5.10x10-6 at 548 K. NH4CI(s)H3(g +HCI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.200 mol NH4CI, 2.26x10-3M NH3 and 2.26x103 M HCI. If the concentration of NH3(g) is suddenly increased to 3.76x10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] [HCI] The equilibrium constant, K, for the following reaction is 10.5...
The equilibrium constant, Ky, for the following reaction is 0.110 at 298 K. NH_HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.50 L container at 298 K contains 2.94 mol of NH_HS(s) and 0.219 mol of NH3(g), the partial pressure of H2S(g) is atm.
2 NH3 (9)+ 3 o2(9) > 3 H20 (9) + NO2 (9) + NO (9) Use the data from this link:ThermodynamicData to calculate the following for the reaction above. (a)AG° at 298 K. kJ (b) Calculate the numerical value of In K at 590 K (c) The temperature at which the reaction can be at equilibrium under standard conditions, if this is possible. If it is not possible, enter 0 (d) The ΔG at 590 K if all reactants in...
Consider the following reaction where K. - 1.80x104 at 298 K. NH, HS()=NH3(g) + H2S(p) A reaction mixture was found to contain 6.00x10-2 moles of NH,HS(s), 1.84x10-2 moles of NH3(8), and 1.34*10-2 moles of H2S(3), in a 1.00 liter container Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse...
and 50. Given the following, determine AGof at 298 K for SnO. Sn(s)+SnO2(s) 2SnO(s); AG° = 12.0 kJ at 298K Substance AGOF(kJ/mol) at 298 K SnO(s) SnO2(s) ? -515.8 95. Consider the following reaction: 3C(s)+4H2(g) -C3H8(g); AH =-104.7 kJ; AS° = -287.4J/K at 298 K What is the equilibrium constant at 400.0 K for this reaction?
The equilibrium constant, K, for the following reaction is 1.30102 at 589 K. NH CH() =NH3(g) + HCI(g) An equilibrium mixture in a 13.0L container at 589 K contains 0.397 mol NH C18), 0.147 M NH3 and 8.84x102 M HCI. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 6.66 L? M ho (NH3] = [HCI) M
For the reaction N2(g) + 3H2(g) = 2 NH3(g), what is AG (in kJ) at 298 K when the pressures of the gases are: P(N2) = .13 atm P(H2) = 6.2 x 10-5 atm P(NH3) = 1.8 atm? +1.73 +47.0 0 -33.0 0-113 0 -2.49
What is AG at 298 K for the following reaction? H2(g) + Brz(9) -2HBr(g): AH = -103.8 kJ; AS = 21.3 J/K at 298 K -110.1 kJ 6.451 * 10 kJ 97.45 kJ -6.451 x 10'
Consider the following system at equilibrium where A1°-268 kJ, and Ke-5.10x10-6, at 548 K. NH4CI(s)NH(g+HCI(g) When some moles of NH4CI(s) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc Kc The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. ○remain the same. It is already at equilibrium. The concentration of NH will
The equilibrium constant, Kc, for the following reaction is 1.80x104 at 298 K. NH_HS(s) ==NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.12 L container at 298 K contains 2.26 mol of NH4HS(s) and 0.282 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining