For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.):
ΔH∘rxn | 179.97 kJ/mol |
ΔS∘rxn | 22.99 J/(mol⋅K) |
Calculate the equilibrium constant for the following reaction at
room temperature, 295.9 K:
Whatever answer you get multiply by 1x1031 and enter that number to 4 decimal places.
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data...
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 185.98 kJ/mol ΔS∘rxn 27.40 J/(mol⋅K) Calculate the temperature in Kelvin above which this reaction is spontaneous. Express your answer to 0 decimal places and in K.
A.) For the decomposition of barium carbonate, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the temperature in kelvins above which this reaction is spontaneous. B.) The thermodynamic values from part A will be useful as you work through part B ΔH∘rxn243.5kJ/mol ΔS∘rxn172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C: BaCO3(s)→BaO(s)+CO2(g)
1. For the reaction of nitric oxide (NO) and oxygen to form nitrogen dioxide, if molecular oxygen is reacting at the rate of 0.00072 M/s, what is the rate (in M/s) of nitric oxide reacting? 2. For the reaction of nitric oxide (NO) and oxygen to form nitrogen dioxide, if molecular oxygen is reacting at the rate of 0.00697 M/s, what is the rate (in M/s) of nitrogen dioxide being formed?
Nitric oxide can be made from the reaction of oxygen and nitrogen gases. O2(g) + N2(g) → 2NO(g) If ΔG° = 165.5 kJ, and ΔH° = 180.4 kJ, what is ΔS° at 325°C? Select one: a. 0.142 kJ/K b. 1.02 kJ/K c. 0.0125 kJ/K d. 0.0458 kJ/K e. 0.0249 kJ/K
the decomposition of nitric oxide to molecular nitrogen and oxygen as shown in the following equation occurs at high temperatures. when the reaction is at equilibrium kc= 0.640 If a sealed 1 L vessel is initially charged with 4.0 mol of NO gas, what is the concentration of NO at equilibrium?
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. b. Determine the temperature(oC) at which the reaction is at equilibrium.
Nitrogen oxide, NO, is a common pollutant produced by the reaction of nitrogen and oxygen gas. Since these gases are several major components of air, nitrogen oxide forms when air is heated in furnaces, engines and other high temperature combustion reactions. Given the standard enthalpy of formation for NO (g) = 90.25 kJ / mole and using the absolute entropies shown in the table below, the free energy change for the reaction at 25.00 ºC can be calculated, and equals...
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. Blank 1 b. Determine the temperature(oC) at which the reaction is at equilibrium.
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) ⇌ 2NO(g) The equilibrium constant Kp for the reaction is 0.31 at 1200 °C. If a container is charged with 0.344 atm of nitrogen and 0.454 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitric oxide? Report your answer to three significant figures
Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N2(9) + 3 H (9) 2NH (9) AH = -92. kJ In the second step, ammonia and oxygen react to form nitric oxide and water: 4 NH (9) + 50,(9) 4 NO(9) + 6H2O(9) AH = -905. kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen,...