The equation of the circle passing through the origin and cutting the circles $x^2 + y^2 + 6x - 15 = 0$ and $x^2 + y^2 - 8y - 10 = 0$ orthogonally is:
\( x^2 + y^2 - 5x + 2y = 0 \)
Step 1: General equation of a circle
The standard equation of a circle is: \[ x^2 + y^2 + 2gx + 2fy + c = 0. \] Since the required circle passes through the origin, substituting \( (0,0) \): \[ 0 + 0 + 2g(0) + 2f(0) + c = 0 \Rightarrow c = 0. \] Thus, the equation simplifies to: \[ x^2 + y^2 + 2gx + 2fy = 0. \]
Step 2: Condition for orthogonality
Two circles cut each other orthogonally if the condition: \[ 2g_1 g_2 + 2f_1 f_2 = c_1 + c_2 \] is satisfied, where \( (g_1, f_1) \) and \( (g_2, f_2) \) are the centres of the two given circles. For the first circle: \[ x^2 + y^2 + 6x - 15 = 0. \] Comparing with \( x^2 + y^2 + 2g_1 x + 2f_1 y + c_1 = 0 \): \[ 2g_1 = 6 \Rightarrow g_1 = 3, \quad f_1 = 0, \quad c_1 = -15. \] For the second circle: \[ x^2 + y^2 - 8y - 10 = 0. \] Comparing: \[ g_2 = 0, \quad 2f_2 = -8 \Rightarrow f_2 = -4, \quad c_2 = -10. \]
Step 3: Apply orthogonality condition
\[ 2g(3) + 2f(0) = -15 + 0. \] \[ 6g = -15 \Rightarrow g = -\frac{5}{2}. \] \[ 2g(0) + 2f(-4) = 0 - 10. \] \[ -8f = -10 \Rightarrow f = \frac{5}{4}. \]
Step 4: Find the required equation
Substituting \( g = -\frac{5}{2} \) and \( f = \frac{5}{4} \) into: \[ x^2 + y^2 + 2gx + 2fy = 0. \] \[ x^2 + y^2 - 5x + 2y = 0. \]
Step 5: Conclusion
Thus, the correct answer is: \[ \mathbf{x^2 + y^2 - 5x + 2y = 0.} \]
In the given figure, the numbers associated with the rectangle, triangle, and ellipse are 1, 2, and 3, respectively. Which one among the given options is the most appropriate combination of \( P \), \( Q \), and \( R \)?

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.