Hydrogen iodide undergoes decomposition according to the equation 2HI(g) = H2(g) + I>(g) The equilibrium constant K, at 500 K for this equilibrium is 0.060. Suppose 0.904 mol of HI is placed in a 5.00-L container at 500 K. What is the equilibrium concentration of I,(g)? (R= 0.0821 L atm/(K - mol)) O 0.082 M O. 0.036 M O 0.044 M O 1.5 M O 0.030 M

Hydrogen iodide undergoes decomposition according to the equation 2HI(g) = H2(g) + I>(g) The equilibrium constant K, at 500 K for this equilibrium is 0.060. Suppose 0.904 mol of HI is placed in a 5.00-L container at 500 K. What is the equilibrium concentration of I,(g)? (R= 0.0821 L atm/(K - mol)) O 0.082 M O. 0.036 M O 0.044 M O 1.5 M O 0.030 M

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.27PAE

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