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19 Nov 2019
Consider the equilibrium
N2(g) + O2(g) â 2 NO(g)
At 2300 K the equilibrium constant K = 1.7 Ã 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species.
*to the right
*to the left
[N2] = ______ mol/L
[O2] = ______ mol/L
[NO] = ______mol/L
Consider the equilibrium
N2(g) + O2(g) â 2 NO(g)
At 2300 K the equilibrium constant K = 1.7 Ã 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species.
*to the right
*to the left
[N2] = ______ mol/L
[O2] = ______ mol/L
[NO] = ______mol/L
Beverley SmithLv2
22 Feb 2019