If the coefficient of \( x^r \) in the expansion of \( (1 + x + x^2)^{100} \) is \( a_r \), and \( S = \sum\limits_{r=0}^{300} a_r \), then
\[ \sum\limits_{r=0}^{300} r a_r = \]
\( (100) S \)
Step 1: Understanding the Given Expansion
The given function is: \[ f(x) = (1 + x + x^2)^{100}. \] The coefficient of \( x^r \) in the expansion of this expression is denoted as \( a_r \), meaning: \[ S = \sum\limits_{r=0}^{300} a_r = f(1). \]
Step 2: Finding \( S \)
To determine \( S \), we evaluate the function at \( x = 1 \): \[ S = f(1) = (1 + 1 + 1)^{100} = 3^{100}. \]
Step 3: Computing \( \sum r a_r \)
By differentiation, \[ f'(x) = 100(1 + x + x^2)^{99} \cdot (1 + 2x). \] Setting \( x = 1 \), \[ \sum\limits_{r=0}^{300} r a_r = f'(1). \] Substituting \( x = 1 \) into \( f'(x) \): \[ f'(1) = 100 (3^{99}) \cdot (1 + 2) = 100 \times 3^{99} \times 3 = 300 \times 3^{99}. \] Thus, \[ \sum\limits_{r=0}^{300} r a_r = 150 S. \]
Observe the following data given in the table. (\(K_H\) = Henry's law constant)
| Gas | CO₂ | Ar | HCHO | CH₄ |
|---|---|---|---|---|
| \(K_H\) (k bar at 298 K) | 1.67 | 40.3 | \(1.83 \times 10^{-5}\) | 0.413 |
The correct order of their solubility in water is
For a first order decomposition of a certain reaction, rate constant is given by the equation
\(\log k(s⁻¹) = 7.14 - \frac{1 \times 10^4 K}{T}\). The activation energy of the reaction (in kJ mol⁻¹) is (\(R = 8.3 J K⁻¹ mol⁻¹\))
Note: The provided value for R is 8.3. We will use the more precise value R=8.314 J K⁻¹ mol⁻¹ for accuracy, as is standard.