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How do the concentrations of reactants and products change over time at equilibrium? 

Consider the endothermic reaction: N2O4(g) 2 NO2(g). Directly after increasing the pressure, what is the relationship between Q and Kc?

Consider the endothermic reaction: N2O4(g) 2 NO2(g)  For our equilibrium, Kc =4.6 * 10-3  under the current conditions. What does this imply for the concentrations of NO2 and N2O4?

The molality of a solution is defined as

What happens to the equation ΔH = ΔU + VΔp if the change in pressure is very small?    

A 1.536 sample of K2SO4 is dissolved in 20.0 g of water (Kf = -1.86oC/m)). The solution freezes at -2.07oC. What is the van’t Hoff factor, i, for this solution?

Calculate the volume of 0.500M stock of Fe3+solution you need to dilute with deionized water to prepare 80.0 mL of 0.0750M solution of Fe3+(aq).

Which substance would lower the freezing point of a solvent the most? 

In the calorimeter experiment that explores the combustion of a fuel, which part of the equation stays constant? ΔH =ΔU + VΔp

Consider the endothermic reaction: N2O4(colorless gas) 2 NO2(brown gas). Why does the color get paler after the pressure increases?