kindly post different questions separately. please rate
2. Calculate K for the reaction: IC (g) at 298 K CH,(g) + 3Cl2(g) = CHCI;(8) + 3HCI(g) at 2 A/Gº(CH.(g)) = -50....
03(g) + OH(g) =H(g) + 2 O2(g) AG° = 5.8 kJ/mol at 298 K, A,Gº = 0 kJ/mol at 354 K, and 4 Gº = -2.0 kJ/mol at 373 K. (a) Calculate the equilibrium constant value for this reaction at 298K, 354 K, and 373 K. (b) At 354K, calculate the change in the Gibbs energy of the reaction, AG when the partial pressures of O3 and OH are kept at 10 bar and 30 bar, respectively, while O2 and...
(3 Points) Calculate the standard Gibbs energy of reaction for the reaction below at 298 K and 596 K. 4 HCl(g) + O2(g) 2Cl2(g) + 2H2O(l) Assume that the heat capacities are constant over the temperature range involved. 02(g) Cl2(g) HCl(g) 4,Hº (kJ mol-4) -92.11 S JK- mol-) 186.91 Comº (K-mol-4) 29.12 AG° (k mol-1) | -95.30 223.07 205.14 9.36 H2O(1) -285.83 69.91 75.29 -237.133 2 33.91
Help (3) For reaction: CH. (g) + 3Cl2(g)at CHCh 01)+3weg). the forward direction has Al603 kJ; and the data below show the of formation, Δ Ge, for each substance at 298-K AG (KJ/mol CH (g) Clh (g) CHCb ( HCI (g) -51 0 -74 -95 (a) Calculate the reaction ΔGo at 298 oK. (b) At standard condition, is the forward reaction spontaneous? And why (c) Calculate the equilibrium constant K1 at 298 °K (d) Calculate the equilibrium constant K2 at...
For the reaction 2 A (g) – B (g), Kp = 0.00565 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
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 reaction and comment on its value. (3 marks) (c) Determine the maximum work done available in the reaction. (3 marks) An equilibrium mixture, consisting of 0.5 atm of NHy(), 0.5 atm of HCKg) and excessive of NH Cl(s), is enclosed in a container at 298 K...
For the reaction 2 A (9) -B (g), Kp = 0.00711 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
a) Calculate K at 298 K for the following reaction: NO(g) + 1 2 O2(g) ? NO2(g) ?G0f(kj/mol) NO(g) 86.60 NO2(g) 51 O2(g) 0 K = ×10
1. Calculate A Gº for the reaction at 25°C 2 SO2(g) + O2(g) → 2 SO3 (g), given that AHº is -197.7 kJ mol- and A.Sº is -188 JK' mol!
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
Calculate Kp at 298 K for the reaction SO.(g) + NO2()SO3(g)+NO() SO2(g) SO3(g) NO(g) NO2(g) -300.4 k/mol -370.4 kJ/mol 86.7 kJ/mol 51.8 kJ/mol For the reaction 2NO(g)+02(g)- 2NO2( f iniially P(NO)1.5 atm, PO2)-1.4 atm, and P(NOJ-2.0 atrn, calculate Δ@for this reaction at 25°C. The following data is valid at 25°C: NO NO2 AGe(kJ/mol 86.7 51.8