Calculate the equilibrium constant, Kp at 500 ℃ for the reaction shown below if the standard enthalpy of reaction, ΔH°rxn = −14.6 kJ/mol at 110 ℃ and the equilibrium constant at this temperature is Kp = 90.2. N2(g) + O2(g) ⇌ 2 NO(g), ΔH = −14.6 kJ/mol R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation. Note: Your answer is assumed to be reduced to the highest power possible.
Calculate the equilibrium constant, Kp at 500 ℃ for the reaction shown below if the standard enthalpy of reaction, ΔH°rxn = −14.6 kJ/mol at 110 ℃ and the equilibrium constant at this temperature is Kp = 90.2. N2(g) + O2(g) ⇌ 2 NO(g), ΔH = −14.6 kJ/mol R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation. Note: Your answer is assumed to be reduced to the highest power possible.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...
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Calculate the equilibrium constant, Kp at 500 ℃ for the reaction shown below if the standard enthalpy of reaction, ΔH°rxn = −14.6 kJ/mol at 110 ℃ and the equilibrium constant at this temperature is Kp = 90.2.
N2(g) + O2(g) ⇌ 2 NO(g), ΔH = −14.6 kJ/mol
R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation.
Note: Your answer is assumed to be reduced to the highest power possible.
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