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À sample of solid NH 4NO 3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s)= N20(g) + 2H20(g) At equilibrium the total pressure in the container was found to be 2.34 atm at a temperature of 500.°C. Calculate Kn. O a. 51.3 O b.1.90 O c. 1.22 Od.0.608 O e. 0.475

À sample of solid NH 4NO 3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s)= N20(g) + 2H20(g) At equilibrium the total pressure in the container was found to be 2.34 atm at a temperature of 500.°C. Calculate Kn. O a. 51.3 O b.1.90 O c. 1.22 Od.0.608 O e. 0.475

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter16: Thermodynamics
Section: Chapter Questions
Problem 50E: Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial...
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A sample of solid NH 4NO 3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s) N2O(g) + 2H2O(g) At equilibrium the total pressure in the container was found to be 2.34 atm at a temperature of 500.°C. Calculate Kn. O a. 51.3 O b.1.90 Oc. 1.22 Od.0.608 O e. 0.475
Transcribed Image Text:A sample of solid NH 4NO 3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s) N2O(g) + 2H2O(g) At equilibrium the total pressure in the container was found to be 2.34 atm at a temperature of 500.°C. Calculate Kn. O a. 51.3 O b.1.90 Oc. 1.22 Od.0.608 O e. 0.475
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