The equilibrium constant Kc for the following reaction is 1.2 at 375 degree C. N2 (g) + H2 (g) <=> 2 NH3 (g) (a) What is the value of KP for this reaction? (b) What is the value of the equilibrium constant Kc for 2 NH3 (g) <=> N2 (g) + 3 H2 (g) (c) What is the value of Kc for 1/2 N2 (g) + 3/2 H2 (g) <=> NH3 (g) ? (d) What are the values of Kp for the reactions described in (b) and (c)?

The equilibrium constant Kc for the reaction H2 (g) + Br2 (g) <=> 2 HBr (g)
is 2.18 $\times$ 10^6 at 730°C. Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.

The equilibrium constant Kc for the reaction 2 NH3 (g) <=> N2 (g) + 3 H2 (g) is 0.83 at 375 degree C. A 14.6-g sample of ammonia is placed in a 4.00-L flask and heated to 375 degree C. Calculate the concentrations of all the gases when equilibrium is reached.

The equilibrium constant Kp for the following reaction is 4.31* 10^(-4) at 375 degree C: N2 + 3 H2 <=> 2 NH3 (g) In a certain experiment a student starts with 0.862 atm of N2 and 0.373 atm of H2 in a constant-volume vessel at 375 degree C. Calculate the partial pressures of all species when equilibrium is reached

All of the halog ens react directly with H2(g) to give binary compounds. The reactions are

$$F2(g) + H2(g)→2 HF(g)$$

.

$$Cl2 (g) + H2 (g)→2 HCl(g)$$

.

$$Brz (g) + H2 (g)→2 HBr (g)$$

.

$$I2(g) + H2 (g)→2 HI (g)$$

Using the data in Appendix D, compute ΔS° of each reaction and identify a periodic trend, if any.

Give three related expressions for the rate of the reaction

$$N2(g)+3H2(g)→2NH3(g)$$

assuming that the concentra tions of any intermediates are constant and that the volume of the reaction vessel does not change.