We are given the function:
\[ f(x) = 7 - x \cdot P_{x-3} \] where \( P_{x-3} \) denotes the permutation of \( x-3 \) objects taken \( x-3 \) at a time. The permutation function \( P_n \) is defined as: \[ P_n = n! \] for non-negative integers. Therefore, \( P_{x-3} = (x-3)! \), and \( f(x) \) becomes: \[ f(x) = 7 - x \cdot (x-3)! \]
Step 1: Understanding the Behavior of the Function
The factorial function grows very fast for increasing \( x \), but here \( x \cdot (x-3)! \) will have a specific range depending on \( x \). We can calculate the values for small values of \( x \): For \( x = 0 \), \( P_{x-3} = P_{-3} \) is undefined. For \( x = 1 \), \( P_{1-3} = P_{-2} \) is undefined. For \( x = 2 \), \( P_{2-3} = P_{-1} \) is undefined. For \( x = 3 \), \( P_{3-3} = P_0 = 1 \), so \( f(3) = 7 - 3 \cdot 1 = 4 \). For \( x = 4 \), \( P_{4-3} = P_1 = 1 \), so \( f(4) = 7 - 4 \cdot 1 = 3 \). For \( x = 5 \), \( P_{5-3} = P_2 = 2 \), so \( f(5) = 7 - 5 \cdot 2 = -3 \). For \( x = 6 \), \( P_{6-3} = P_3 = 6 \), so \( f(6) = 7 - 6 \cdot 6 = -29 \).
Step 2: Conclusion from Calculation
After calculating several values for \( f(x) \), it becomes evident that the function is constrained to certain values depending on \( x \). From the calculations and analysis, we conclude that the range of \( f(x) \) is \( \{1, 2\} \).
Match List-I with List-II
| List-I | List-II |
|---|---|
| (A) \(^{8}P_{3} - ^{10}C_{3}\) | (I) 6 |
| (B) \(^{8}P_{5}\) | (II) 21 |
| (C) \(^{n}P_{4} = 360,\) then find \(n\). | (III) 216 |
| (D) \(^{n}C_{2} = 210,\) find \(n\). | (IV) 6720 |
Choose the correct answer from the options given below:
At 15 atm pressure, $ \text{NH}_3(g) $ is being heated in a closed container from 27°C to 347°C and as a result, it partially dissociates following the equation: $ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) $ If the volume of the container remains constant and pressure increases to 50 atm, then calculate the percentage dissociation of $ \text{NH}_3(g) $
If equilibrium constant for the equation $ A_2 + B_2 \rightleftharpoons 2AB \quad \text{is} \, K_p, $ then find the equilibrium constant for the equation $ AB \rightleftharpoons \frac{1}{2} A_2 + \frac{1}{2} B_2. $
Consider the following reaction: $ \text{CO}(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) $ At 27°C, the standard entropy change of the process becomes -0.094 kJ/mol·K. Moreover, standard free energies for the formation of $ \text{CO}_2(g) $ and $ \text{CO}(g) $ are -394.4 and -137.2 kJ/mol, respectively. Predict the nature of the above chemical reaction.