23. The rate constant for a particular reaction is 27 activation energy for the reaction in...
25. A mixture of 0.100 mol of NO, 0.0500 mol of H2, and 0.100 mol of H2O is placed in a 1.00-L vessel. The following equilibrium is established: 2NO(g) + 2H2 (g) → N2(g) + 2H2O(g) At equilibrium [NO] -0.0620 M. Calculate the equilibrium concentrations of H2, N2, and H20.
23. The rate constant for a particular reaction is 2.7 x 10-2 s at 25°C and 6.2 x 102 s at 75°C. What is the activation energy for the reaction in kJ/mol? (R-8.314 J/mol.K)
For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g), what direction will the reaction proceed if [NO]=7.9x10-3M, [H2]=0.25 M, [N2]=0.15 M, & [H2O]=0.13 M. (K=650) forward reverse the reaction has stopped the reaction is at equilibrium
the following reaction 2NO(0) + 2H2 (g) № (g) + 2 HaO (g) H2/0000 M quilbrium constant, Ke, for the reaction. Initially, a mixture of 0.300 M NO, 0.100 M NOwas found to beg,062-м. D.ig2 the value of the brium (init h N2)t eubrhum the conentreton dr H20 was allowed to reach equilibrium ( 0-200 8) Consider the following reaction. HSO.. (aq) + H2O (I) → HO. (aq) + SO2-(aq) The initial concentrations are [HSO門-0.3000 M, [HO+]s 0.050 M. [SO...
________________________________________________________________ ________________________________________________________________________ The equilibrium-constant expression for a gas reaction is [N, H4] [N][H,12 Choose the balanced chemical equation corresponding to this expression. N2(g) + 2H2 (9) = N2H (9) ON, H. (g) = N2(g) + 2H2 (9) N2(9) + H2(9) N2H4(9) 2N2 (9) + 4H2(g) = 2N, H4 (9) Iodine and bromine react to give iodine monobromide, IBr. 12 (9) + Br2(g) = 21Br(9) What is the equilibrium composition of a mixture at 126°C that initially contained 1.30 x 10...
The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M⁻¹s⁻¹, then what is the value of the rate constant at 209 °C? (R = 8.314 J/mol • K)
The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M⁻¹s⁻¹, then what is the value of the rate constant at 121 °C? (R = 8.314 J/mol • K)
The rate law for the reaction 2H2(g) + 2NO(g) ----> N2(g) + 2H2O(g) is rate=k[H2][NO]2. What is the rate constant at 800 degrees C when [NO] = 0.050 M and [H2] = 0.010 M and the rate of the reaction is 1.5 M/s
what is the correct rate law for the reaction at 1500 C determine the rate constant for the reaction at 1500C Hydrogen gas reduces NO to N2 in the following reaction: 2H2 (g) +2NO(&2H20(g)N2() The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2lo (M) [NOlo (M) Initial Rate (M/s) 2 3 4 0.212 0.212 0.424 0.848 0.136 0.272 0.544 0.544 0.0265 0.0533 0.419 1.68
Calculate the activation energy for the reaction 2NOCl = 2NO + Cl, if the rate constant k is equal to 0.286 L/mol*s at 500 K and 0.175 L/mol*s at 490 K.