One mole of solid NH4Cl (s) isvheated in a closed box to decompose it partially according to the following reaction: 

NH4Cl (s) <=> NH3 (g) +HCl (g)

 A) calculate Kp of the above system at the temperature of the experiment if the partial pressure of ammonia at equilibrium is 1.6atm.
B) what happens to Kp and the partial pressure of HCl (g) if:
 -some NH3 gas is pumped into the box at same T.
 -More NH4Cl is added without changing T
 -the volume of the box is reduced 50% at same T.

A) To calculate Kp for the given reaction, we need to know the equilibrium concentrations of NH3 and HCl gases. Since we are given the partial pressure of ammonia (NH3) at equilibrium (1.6 atm), we can use that information to calculate Kp.

The expression for Kp is given by:

Kp = (P(NH3) * P(HCl)) / P(NH4Cl)

Since the reaction is in a closed box, we assume the total pressure is constant and equal to the sum of the partial pressures:

P(NH3) + P(HCl) + P(NH4Cl) = constant

However, since we don't have the values for P(HCl) or P(NH4Cl), we cannot directly calculate Kp with the given information. We need additional data such as the partial pressure of HCl or the equilibrium concentration of NH4Cl to find the equilibrium concentrations of the other gases and then calculate Kp.

B) Let's analyze the effects of the given scenarios on Kp and the partial pressure of HCl (g):

- If some NH3 gas is pumped into the box at the same temperature (T), the reaction will shift to the left to consume the additional NH3. This means that the concentration of NH4Cl will increase, resulting in an increase in the partial pressure of HCl (g). However, without knowing the specific values or concentrations, we cannot determine the exact effect on Kp.

- If more NH4Cl is added to the box without changing the temperature (T), the reaction will shift to the right to consume the additional NH4Cl. This will result in an increase in the concentration of NH3 and HCl, thus increasing their partial pressures. Again, without specific values or concentrations, we cannot determine the exact effect on Kp.

- If the volume of the box is reduced by 50% at the same temperature (T), the partial pressures of both NH3 and HCl will increase. This is because reducing the volume increases the concentration of the gases, causing the reaction to shift towards the side with fewer moles of gas (right side in this case). As a result, the partial pressure of HCl (g) will increase as well. However, the effect on Kp depends on the equilibrium concentrations of NH3 and HCl, which are not given.

In summary, without knowing specific numeric values or concentrations, we cannot determine the exact impact on Kp or the partial pressure of HCl (g) for the given scenarios.