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

Consider the endothermic reaction: N2O4(g) 2 NO2(g).  How the equilibrium is affected by an increase in temperature?

After the following solutions reacted at the conditions different from your experiment, the measured absorbance was  0.245. Use the calibration equation from your lab report to fill Tables 1 and 2. Embed your calculations to the Exam Calculations for 5 pts after you submitted this exam Table 1 Rice Table ( 12pts) Volume of 0.0020 M Fe(NO3)3 solution Volume of 0.0020 M KSCN solution Volume of 0.300 M HNO3 solution [Fe3+] initial [SCN-] initial [Fe(SCN)2+] equilibrium [Fe3+]  equilibrium [SCN-]  equilibrium Ка 5.00 mL 2.00 mL 3.00 mL Table 2 Rice Table ( 8pts) Reaction Fe3+(aq) + SCN−(aq) ⇌ FeSCN2+(aq Initial concentration, M (mol/L) Change in concentration at equilibrium, M Equilibrium concentration, M: Embed your calculations for both tables to the Exam Calculations for 5 pts after you submitted this exam

What is the concentration of the following compound as measured in a 1 cm cuvette: Molar absorptivity: 2525/M*cm. Absorption: 0.4322. Attention: SigFig

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

Which equation do we need to find out how many moles of NH4Cl are in the solution?

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?

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

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

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