We know that
ln(K2/K1) = -delta H/R (1/T2-1/T1)
ln (0.53/0.45) = - delta H/8.314 (1/(273+90) -1/(273+40)
0.164 = -delta H/8.314 (-4.4 x 10-4)
1.36 = delta H * 4.4 x 10-4
delta H = 3098 = 3.098 kJ
If K_c = 0.450 at 40.degree C and K_c = 0.530 at 90.degree C, what is...
For the reaction N_2 + 3h_2(g) <===> 2NH_3 (g) at 90 degree C, K_c = 1.27 times 10^-3 Determine K_p for this system. R = 0.08206 L -atm/(mol-K)
The equilibrium constant K_c for the following equation at 900 degree C is 27.8. What is the value for K_c for the following equation?
An aqueous reaction at 350 K has an equilibrium constant (K_c) of 2.65 times 10^-6. What is the delta G degree of the reaction at 350 K?
If Kc = 0.440 at 40.°C and Kc = 0.515 at 90.°C, what is ΔH° for the reaction? X <---> Y
The vapor pressure of water at 25 degree C is o.0313 atm. Calculate the values of K_p and K_c at 25 degree C for the equilibrium: H_2O (l) H_2O(g). Vinegar contains acetic acid, a weak acid that is partially dissociated in aqueous solution: CH_3COOH(aq) H^+(aq) + CH_3CO^-_2 (aq) a) Write the equilibrium constant expression for K_c. b) What is the value of K_c if the extent of dissociation of 1.0 M CH_3COOH is 0.42%? Determination of an Equilibrium Constant
25. What is the potential 0.530 x 10-40 m from a proton (the average distance between the proton and electron in a hydrogen atom)?
Use the data given here to calculate the values of delta G^degree _rxn at 25^degree C for the reaction described by the equation A + B double headed arrow C If delta D^degree _rxn and delta S^degree _rxn are both negative values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is entropy-driven to the right. entropy-driven to the left. enthalpy-driven to the left. enthalpy-driven to the right.
Chemistry help
Calculate delta H degree and Delta G degree following reactions at 25 degree C, using thermodynamic data from Appendix C; interpret the signs of Delta H degree and Delta G degree. (18.50) 2PbO(s) + N_2(g) rightarrow 2Pb(s) + 2NO(g) CS_2(I) + 2H_2O(l) rightarrow CO_2(g) + 2H_2S(g)
Calculate the standard entropy, Delta S_rxn^degree, of the following reaction at 25.0 degree C using the data in this table. The standard enthalpy of the reaction, Delta H_rxn^degree, is -633.1 kJ middot mol^-1. 3C_2 H_2(t) rightarrow C_6 H_6 (l) Delta S_rxn^degree = Number J middot K^-1 middot mol^-1 Then, calculate the standard Gibbs free energy of the reaction, Delta G_rxn^degree. Delta G_rxn^degree = Number kJ middot mol^-1 Finally, determine which direction the reaction is spontaneous as written at 25.0 degree...
If Kc = 0.460 at 40.°C and Kc = 0.685 at 90.°C, what is ΔH° for the reaction?