Statement-1 : Ammonia at a pressure of 10 atm and `CO_(2)` at a pressure of 20 atm are intoduced into an evacuated chamber. If Kp for the reaction.
`NH_(2)COONH_(4)(s) 2NH_(3)(g) + CO_(2)(g)` is 2020 `atm^(3)`, the total pressure after a long time is less than 30 atm.
Statement-2 : Equilibrium can be attained from both directions.

Options

A. Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1
B. Statement-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1
C. Statement-I is false, statement-2 is true.
D. Statement-1 is true, statement-2 is false.

Answer

To solve the problem, we will analyze the given statements step by step.

### Step 1: Understand the Reaction
The reaction given is:
\[ \text{NH}_2\text{COONH}_4 (s) \rightleftharpoons 2 \text{NH}_3 (g) + \text{CO}_2 (g) \]
This indicates that solid ammonium carbamate decomposes into gaseous ammonia and carbon dioxide.

### Step 2: Initial Conditions
We are given:
- Initial pressure of ammonia, \( P_{\text{NH}_3} = 10 \, \text{atm} \)
- Initial pressure of carbon dioxide, \( P_{\text{CO}_2} = 20 \, \text{atm} \)

Thus, the total initial pressure is:
\[ P_{\text{total}} = P_{\text{NH}_3} + P_{\text{CO}_2} = 10 \, \text{atm} + 20 \, \text{atm} = 30 \, \text{atm} \]

### Step 3: Equilibrium Constant
The equilibrium constant \( K_p \) for the reaction is given as:
\[ K_p = 2020 \, \text{atm}^3 \]
This means at equilibrium, the ratio of the partial pressures of the products raised to their stoichiometric coefficients will equal \( K_p \).

### Step 4: Reaction Direction
Since \( K_p \) is a large value, it indicates that at equilibrium, the formation of products (NH3 and CO2) is favored. However, if we start with more products than the equilibrium constant suggests, the reaction will shift to the left, favoring the formation of solid NH2COONH4.

### Step 5: Total Pressure After a Long Time
As the reaction proceeds towards equilibrium, some of the gaseous products will convert back into the solid reactant. This means that the total pressure will decrease because the solid does not contribute to the pressure in the gas phase.

Thus, after a long time, the total pressure will indeed be less than the initial total pressure of 30 atm.

### Conclusion for Statement 1
Statement 1 is true: The total pressure after a long time is less than 30 atm.

### Step 6: Analyzing Statement 2
Statement 2 states that equilibrium can be attained from both directions. This is true because the reaction can proceed both forwards (solid to gas) and backwards (gas to solid).

### Conclusion for Statement 2
Statement 2 is also true, but it does not explain why the total pressure decreases in Statement 1. Therefore, while both statements are true, Statement 2 is not the correct explanation for Statement 1.

### Final Answer
- Statement 1 is true.
- Statement 2 is true, but it is not the correct explanation for Statement 1.

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