Answer - 0.11NH4HS(s) -------------------NH3(g) + H2S(g)start at 0.5atm . 0atmequilibrium 0.5 + xatm xatmThen 0.5 + x + x = 2x + 0.5 = 0.84 (given) ----x=0.17atmPNH3 = 0.5 + 0.17 = 0.67atm, PH2S = 0.17atmK = PNH3 X PH2S = 0.67 X 0.17 = 0.1189= 0.11

NH4HS(s)->NH3(g)+H2S(g)initial 0.5 0at eq 0.5+x xTotal pressure=0.5+x+x=0.84(given)2x=0.34...we get x=0.17now PNH3=0.5+x=0.5+0.17=0.67aatmPH2S=x=0.17atmEquilibrium constant =[PNH3][PH2S]=0.67×0.17=0.11Kc=o.11here while writing eq constant we doesnot include NH4HS...as it is a solid...jyotsna is crct...HOPE U GOT IT

Equilibrium Constant for the Decomposition Reaction of NH4HS

To determine the equilibrium constant for the decomposition of NH4HS, we need to understand the balanced chemical equation for the reaction and how the total pressure in the flask changes at equilibrium.

1. Balanced Chemical Equation

The decomposition reaction of NH4HS can be represented by the following balanced chemical equation:

NH4HS(s) ⇌ NH3(g) + H2S(g)

From the equation, we can see that one mole of NH4HS decomposes to yield one mole of NH3 gas and one mole of H2S gas.

2. Initial Conditions

Initially, the flask contains solid NH4HS and ammonia gas at a certain temperature and 0.50 atm pressure. This means that the initial partial pressure of NH3 is 0.50 atm.

3. Equilibrium Conditions

At equilibrium, the total pressure in the flask rises to 0.84 atm. This total pressure is the sum of the partial pressures of NH3 and H2S gases.

Let's assume that at equilibrium, the partial pressure of NH3 is P1 and the partial pressure of H2S is P2.

Therefore, we can write the following equation based on the given information:

P1 + P2 = 0.84 atm

4. Relationship between Pressure and Concentration

According to the ideal gas law, the pressure of a gas is directly proportional to its concentration. Therefore, we can write the following equation:

P = nRT/V

Where:
P = pressure
n = moles of gas
R = ideal gas constant
T = temperature
V = volume

5. Equilibrium Constant Expression

The equilibrium constant expression can be derived using the balanced chemical equation and the relationship between pressure and concentration.

Since the coefficients in the balanced equation are 1 for all species, the equilibrium constant expression can be written as:

K = (P1 * P2) / (P(NH4HS))

Where:
K = equilibrium constant
P1 = partial pressure of NH3
P2 = partial pressure of H2S
P(NH4HS) = partial pressure of NH4HS (initial pressure of ammonia gas)

6. Solving for the Equilibrium Constant

Using the given information and the equation P1 + P2 = 0.84 atm, we can substitute the values into the equilibrium constant expression:

K = (P1 * P2) / (0.50 atm)

Simplifying further:

K = (P1 * P2) / 0.50

Since the equilibrium constant is a dimensionless quantity, the units of pressure cancel out.

7. No Numerical Values Provided

Unfortunately, we don't have any numerical values for the partial pressures of NH3 and H2S, so we cannot calculate the exact equilibrium constant.

However, based on the given information and the equilibrium condition, we can conclude that the equilibrium constant for the decomposition of NH4HS at the given temperature is greater than 1. This is because the total pressure in the flask increases from the initial 0.50 atm to 0.84 atm at equilibrium.

Summary

In summary, the equilibrium constant for the decomposition of NH4HS at the given temperature can be determined by