The equilibrium constant for the reaction NO(g) + O2(g) <=> 2NO2(g) decreases from 1.5 x 105 at 430ºC to 23 at 1000ºC. From these data, calculate the value of ΔHº for the reaction. ΔHº = _________ kJ/mol.
The equilibrium constant for the reaction NO(g) + O2(g) <=> 2NO2(g) decreases from 1.5 x 105 at 430ºC to 23 at 100...
Be sure to answer all parts. At 430°C, the equilibrium constant (Kp) for the reaction 2NO(g)+O2()s 2NO2(g) is 1.5 x 105. In one experiment, the initial pressures of NO, O2, and NO are 6.3 x 103 atm, 1.9 x 10-2 atm, and 0.18 atm, respectively. Calculate Op and predict the direction that the net reaction will shift to reach equilibrium. What is Qp for the experiment? 4.29 In which direction will the system proceed to reach equilibrium? The reaction will...
The equilibrium constant KcKc for the reaction 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) is 6.9×1056.9×105 at 500 KK. A 5.0 LL reaction vessel at 500 KK was filled with 0.052 molmol of NONO, 1.1 molmol of O2O2, and 0.90 molmol of NO2NO2. Part A What is the value of QcQc? Express your answer to two significant figures.
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
Calculate the value of the equilibrium constant for the reaction N2(g) + 2O2(g) ⇌ 2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0011, [O2] = 0.0033, and [NO2] = 0.0048. Keq = _______________
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperatures: Kp: 170K 3.8*10^-3 180K 0.34 190K 18.4 200K 681 Part A Use the data to find ΔH∘rxn and ΔS∘rxn for the reaction. i found ΔH∘rxn = 114 kJ but i dont know how to get ΔS∘rxn. please help and show work
Thermodynamics Free energy and chemical equilibrium Quiz: Te equilibrium constant for the reaction Na + O2 + 2 NO 200 Decreases from 1.5-10 at 430 °C to 23 at 1000°C. From these data: a - calculate enthalpy change of this reaction; b-equilibrium constant at 1500 °C
problem #9 Calculate the equilibrium constant for the following reaction at 25°C. 2H2(g) + O2(g) 2H20cv) Given the following standard free-energy: H2O , -237.2 KJ/mol at 25°C. Problem #10. Given the following data at 25°C: substance sº (J/mol.K) AH', (KJ/mol) 240.45, 33.8 304.33 9.66 NO 249) N2O160) (a) Calculate the value of A Gº for the following reaction at 25°C: 2 NO2(9) N20 (9) (b) Is the formation of NO a spontaneous process at 25°C and standard-state conditions? (a) What...
. Determine the value of the equilibrium constant for the reaction N2 (g) + 2O2 (g) ↔ N2O4 (g) from the following equations. ½ N2 (g) + ½ O2 (g) ↔ NO (g) KC = 6.9 x 10-16 2NO2 (g) ↔ 2NO (g) + O2 (g) KC = 4.5 x 10-13 2NO2 (g) ↔ N2O4 (g) KC = 6.7
2- For the reaction 2NO(g) + O2(g)2NO2(g) H° = -114.2 kJ and S° = -146.5 J/K The equilibrium constant for this reaction at 289.0 K is ---------- . Assume that H° and S° are independent of temperature.