1. Consider the following equilibrium at T = 298 K and P = 1.0 atm:

A B

The equilibrium constant, K_eq, under these conditions is 1.6 x 10^-4. Imagine mixing together 1.0 mole of A and 1.0 mole of B in a reaction flask. At the instant of mixing (before the reaction starts), what must happen for the mixture to reach equilibrium, and what is true about the reaction quotient, Q?

a.Nothing; Q = K

b.A will react to make more B; Q > K

c.Cannot determine based on the information given

d.A will react to make more B; Q < K

e.B will react to make more A; Q < K

f.B will react to make more A; Q > K

2. A chemical reaction has Hrxn=15.76 kJ/mol and Srxn= 15.68 J K^-1 mol^-1 at T = 298 K and P = 1.0 bar. Assume that Hrxnand Srxn are independent of temperature. A van't Hoff plot shows how the equilibrium constant, K, varies with temperature. It is plotted with lnK on the y-axis, and 1/T on the x-axis.Calculate the slope, m, of the line of best fit on the van't Hoff plot for this reaction.

3. A chemical reaction has H= 8.9 kJ mol^-1 and an equilibrium constant of 4.4 at T = 298 K.

Assuming that H is constant over the temperature range in question, what is the equilibrium constant at T = 347.4 K?