Nitrogen oxide, NO, is a common pollutant produced by the reaction of nitrogen and oxygen gas....
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 _______ kJ. The sign also tells us this reaction (is/ is not) ____________ favored at 25 degrees C.
| Entropy ( S º ) | |
| N2 (g) | 191.5 J / ( mol K ) |
| NO (g) | 210.7 J / ( mol K ) |
| O2 (g) | 205.0 J / ( mol K ) |
Homework Answers
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Nitrogen oxide, NO, is a common pollutant produced by the
reaction of nitrogen and oxygen gas....
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power...
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power plants according to the reaction N2 (g)+02 (g) 2NO (g) A constant-volume reactor of 100 L is initially charged with 4 mol of N2 and 1 mol of O2 and then temperature is increased to 800 K. Estimate the equilibrium extent of the reaction if the pressure is kept constant at 1 bar (Answer: 5.567 x 10-6)
The pollutant NO is formed in diesel engines. The reaction fixes atmospheric nitrogen with oxygen to...
The pollutant NO is formed in diesel engines. The reaction fixes atmospheric nitrogen with oxygen to form NO. The reaction is: N2(g) + O2(g) = 2NO(g). If the equilibrium constant for this reaction at elevated temperatures is 5.60E-11, then what is the partial pressure of NO gas if nitrogen is 1.50 atm and oxygen is 0.500 atm? The units are atmospheres.
7. Nitrogen dioxide is formed from nitrogen monoxide and oxygen in a product favored reaction at...
7. Nitrogen dioxide is formed from nitrogen monoxide and oxygen in a product favored reaction at 25°C. Determine the standard entropy change AS, for the reaction AS9rxn (=AS sys). AS for NO2 is 240.1 JK' mol!. As for NO is 210.8 JK 'mol!, AS for O2 is 205.1 J K mol'. Remember to scale each entropy value by the number of moles of reactant or product involved.
6. If 1.4 g of nitrogen is reacted with excess oxygen in a calorimeter containing 254...
6. If 1.4 g of nitrogen is reacted with excess oxygen in a calorimeter containing 254 g of water (specific heat capacity: 4.18 J/g·K), the temperature of the water changes from 25.0 ºC to 23.4 ºC. Determine the value of delta H (in kJ/mol) for this reaction per mole of nitrogen. N2(g) + 2 O2(g) N2O4(g) a. 1.2 kJ b. 1.7 kJ c. 17 k J d. 34 kJ
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.
An important reaction in combustion processes is the gas phase oxidation of CO, a poisonous gas...
An important reaction in combustion processes is the gas phase oxidation of CO, a poisonous gas and pollutant CO+1/2O2=CO2 Delta rxn H(298k)=-283 kj/mol; Delta rxn G(298k)=-257.2 kj/mol A.) Is the reaction favored at 298k? Explain B.) How will the molar extent of reaction change as the temperature is increased at constant pressure? Estimate the temperature at which the molar extent of reaction is 0.9855 at 1 Bar total pressure. Assume ideal gases and heat of reaction to be independent of...
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 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.
Nitrogen monoxide is a pollutant in the lower atmosphere that irritates the eyes and lungs and...
Nitrogen monoxide is a pollutant in the lower atmosphere that irritates the eyes and lungs and leads to the formation of acid rain. Nitrogen monoxide forms naturally in the atmosphere according to the endothermic reaction: N2(g) + O2(g) ----> 2 NO(g) Kp = 4.1 * 10-31 at 298 K Use the ideal gas law to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 atm and a temperature at 298 K. Assume that nitrogen...
Use the standard molar entropies B to calculate the standard entropy of reaction for the oxidation...
Use the standard molar entropies B to calculate the standard entropy of reaction for the oxidation of graphite to carbon monoxide: 2C(s)+O2(g)→2CO(g) C(s) = 5.7 J/K*mol, O2(g) = 205.0 J/K*mol, CO(g)= 197.6 J/K*mol Express your answer using one decimal place and include the appropriate units.
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) →...
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). Species ΔH°f, kJ/mol S°, J/(K · mol) NO (g) 91.3 210.7 O2 (g) 0.0 205.0 NO2 (g) 33.2 240.0 A) -157.8 kJ B) -532.6 kJ C) -72.6 kJ D) -4.7 kJ
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power plants according to the reaction N2 (g)+02 (g) 2NO (g) A constant-volume reactor of 100 L is initially charged with 4 mol of N2 and 1 mol of O2 and then temperature is increased to 800 K. Estimate the equilibrium extent of the reaction if the pressure is kept constant at 1 bar (Answer: 5.567 x 10-6)
7. Nitrogen dioxide is formed from nitrogen monoxide and oxygen in a product favored reaction at 25°C. Determine the standard entropy change AS, for the reaction AS9rxn (=AS sys). AS for NO2 is 240.1 JK' mol!. As for NO is 210.8 JK 'mol!, AS for O2 is 205.1 J K mol'. Remember to scale each entropy value by the number of moles of reactant or product involved.
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