3 - phases. Ca(HCO3)2(aq) ' CaCO3(s) + H2O(l) + CO2(g)...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Q for a reaction is the ratio of concentrations of products to concentrations of reactants. As the reaction progresses the concentration of reactants decrease and the concentration of products increase, which means that Q increases as a function of time. The value of Q increases as a function of time until it reaches the value of K. b) No, Q would still increase with time because the [I2] would decrease in exactly the same way as [H2] decreases. 17.9 A homogeneous equilibrium reaction exists when all the components of the reaction are in the same phase (i.e., gas, liquid, solid, aqueous). 2 NO(g) + O2(g) ' 2 NO2(g) A heterogeneous equilibrium reaction exists when the components of the reaction are in different
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: phases. Ca(HCO3)2(aq) ' CaCO3(s) + H2O(l) + CO2(g) 17.10 1/2 N2(g) + 1/2 O2(g) ' NO(g) Qc(form) NO(g) ' 1/2 N2(g) + 1/2 O2(g) , so the constants do differ (they are the reciprocal of each other). 17.11 Yes, the Qs for the two reactions do differ. The balanced equation for the first reaction is 3/2 H2(g) + 1/2 N2(g) ' NH3(g) (1) The coefficient in front of NH3 is fixed at 1 mole according to the description. In the second reaction, the coefficient in front of N2 is fixed at 1 mole. 3 H2(g) + N2(g) ' 2 NH3(g) (2) The reaction quotients for the two equations and their relationship are: 3 3 1...
View Full Document

This note was uploaded on 03/14/2012 for the course CHEN 654 taught by Professor Nimos during the Winter '12 term at Beaufort County Community College.

Ask a homework question - tutors are online