4
The power of a point \( (x_1, y_1) \) with respect to a circle \( (x - h)^2 + (y - k)^2 = r^2 \) is given by the formula: \[ P = (x_1 - h)^2 + (y_1 - k)^2 - r^2 \] For the point \( (0, 2) \) and the power 4: \[ (0 - h)^2 + (2 - k)^2 - r^2 = 4 \] This simplifies to: \[ h^2 + (2 - k)^2 - r^2 = 4 \quad \text{(Equation 1)} \] The circle passes through the points \( (2, 0) \) and \( (1, 2) \). These points must satisfy the circle's equation \( (x - h)^2 + (y - k)^2 = r^2 \). Therefore, we have the following two equations: 1. For point \( (2, 0) \): \[ (2 - h)^2 + (0 - k)^2 = r^2 \] This simplifies to: \[ (2 - h)^2 + k^2 = r^2 \quad \text{(Equation 2)} \] 2. For point \( (1, 2) \): \[ (1 - h)^2 + (2 - k)^2 = r^2 \] This simplifies to: \[ (1 - h)^2 + (2 - k)^2 = r^2 \quad \text{(Equation 3)} \] Step 1: Solving the system of equations From Equation 2: \[ (2 - h)^2 + k^2 = r^2 \] Expanding: \[ 4 - 4h + h^2 + k^2 = r^2 \quad \text{(Equation 4)} \] From Equation 3: \[ (1 - h)^2 + (2 - k)^2 = r^2 \] Expanding: \[ 1 - 2h + h^2 + 4 - 4k + k^2 = r^2 \] Simplifying: \[ 5 - 2h - 4k + h^2 + k^2 = r^2 \quad \text{(Equation 5)} \] Step 2: Substitute the values from Equations 4 and 5 We can now substitute the expression for \(r^2\) from Equation 4 into Equation 5 and solve for \(h\) and \(k\). Step 3: Calculate the radius After solving the system of equations for \( h \), \( k \), and \( r \), we find the radius of the circle to be: \[ r = \sqrt{\frac{5}{2}} \] Thus, the radius of the circle is \( \boxed{\sqrt{\frac{5}{2}}} \).
What is the angle between the hour and minute hands at 4:30?
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.