Step 1: Understanding the Given Expression
We are given the expression: \[ \lim_{x \to 0^+} \frac{\cos^{-1}(1 - \{x\}^2) \sin^{-1}(1 - \{x\})}{\{x\} - \{x\}^3} = \theta \] where \( \{x\} \) denotes the fractional part of \( x \), i.e., \( \{x\} = x - \lfloor x \rfloor \). As \( x \to 0^+ \), we know that \( \{x\} \to 0 \) since the fractional part of \( x \) becomes very small as \( x \) approaches 0 from the positive side. We are asked to find the value of \( \tan(\theta) \).
Step 2: Approximation of Functions
As \( x \to 0^+ \), we have \( \{x\} \to 0 \). Therefore, we can use small angle approximations for the inverse trigonometric functions. For small values of \( y \), we know: \[ \cos^{-1}(1 - y^2) \approx \sqrt{2y} \] and \[ \sin^{-1}(1 - y) \approx \sqrt{2y} \] Thus, for \( \{x\} \) being small, we have: \[ \cos^{-1}(1 - \{x\}^2) \approx \sqrt{2\{x\}} \] and \[ \sin^{-1}(1 - \{x\}) \approx \sqrt{2\{x\}} \]
Step 3: Substituting the Approximations into the Expression
Now, substitute these approximations into the given expression: \[ \frac{\cos^{-1}(1 - \{x\}^2) \sin^{-1}(1 - \{x\})}{\{x\} - \{x\}^3} \approx \frac{(\sqrt{2\{x\}})(\sqrt{2\{x\}})}{\{x\} - \{x\}^3} \] This simplifies to: \[ \frac{2\{x\}}{\{x\} - \{x\}^3} \]
Step 4: Simplifying the Expression
For small \( \{x\} \), we can neglect \( \{x\}^3 \) in comparison to \( \{x\} \). Therefore, the denominator simplifies to \( \{x\} \). The expression now becomes: \[ \frac{2\{x\}}{\{x\}} = 2 \] Thus, we have: \[ \theta = 2 \]
Step 5: Final Calculation
We are asked to find \( \tan(\theta) \). Since \( \theta = 2 \), we compute: \[ \tan(2) \approx \sqrt{3} \] Therefore, the value of \( \tan(\theta) \) is \( \sqrt{3} \).
Step 6: Final Answer
The correct answer is: \[ \boxed{\sqrt{3}} \]
For $ \alpha, \beta, \gamma \in \mathbb{R} $, if $$ \lim_{x \to 0} \frac{x^2 \sin \alpha x + (\gamma - 1)e^{x^2} - 3}{\sin 2x - \beta x} = 3, $$ then $ \beta + \gamma - \alpha $ is equal to:
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.