\(\frac{1}{\sqrt{7}}(8\mathbf{i} - 5\mathbf{j} + 3\mathbf{k})\)
Step 1: Find the position vector of \(C\) using the section formula. Since \(C\) divides \(AB\) in the ratio \(3:2\), we use the section formula to find the position vector of \(C\): \[ \mathbf{C} = \frac{2\mathbf{A} + 3\mathbf{B}}{5} \] Substitute the position vectors of \(A\) and \(B\): \[ \mathbf{C} = \frac{2(2\mathbf{i} - 3\mathbf{j} + \mathbf{k}) + 3(\mathbf{i} + 2\mathbf{j} - 3\mathbf{k})}{5} \] \[ \mathbf{C} = \frac{(4\mathbf{i} - 6\mathbf{j} + 2\mathbf{k}) + (3\mathbf{i} + 6\mathbf{j} - 9\mathbf{k})}{5} \] \[ \mathbf{C} = \frac{7\mathbf{i} - 7\mathbf{k}}{5} \] Thus, the position vector of \(C\) is: \[ \mathbf{C} = \frac{7}{5}\mathbf{i} - \frac{7}{5}\mathbf{k} \]
Step 2: Find the vector \( \mathbf{CD} \). The vector \( \mathbf{CD} \) is found by subtracting the position vector of \(C\) from the position vector of \(D\): \[ \mathbf{CD} = \mathbf{D} - \mathbf{C} = (3\mathbf{i} - \mathbf{j} + 2\mathbf{k}) - \left(\frac{7}{5}\mathbf{i} - \frac{7}{5}\mathbf{k}\right) \] \[ \mathbf{CD} = \left(3 - \frac{7}{5}\right)\mathbf{i} - \mathbf{j} + \left(2 - \left(-\frac{7}{5}\right)\right)\mathbf{k} \]
Step 3: Find the magnitude of \( \mathbf{CD} \). The magnitude of \( \mathbf{CD} \) is: \[ |\mathbf{CD}| = \sqrt{\left(\frac{8}{5}\right)^2 + (-1)^2 + \left(\frac{17}{5}\right)^2} \] \[ |\mathbf{CD}| = \sqrt{\frac{64}{25} + 1 + \frac{289}{25}} = \sqrt{\frac{64 + 25 + 289}{25}} = \sqrt{\frac{378}{25}} = \frac{\sqrt{378}}{5} = \frac{3\sqrt{42}}{5} \]
Step 4: Find the unit vector in the direction of \( \mathbf{CD} \). The unit vector in the direction of \( \mathbf{CD} \) is: \[ \hat{\mathbf{CD}} = \frac{\mathbf{CD}}{|\mathbf{CD}|} = \frac{\frac{8}{5}\mathbf{i} - \mathbf{j} + \frac{17}{5}\mathbf{k}}{\frac{3\sqrt{42}}{5}} = \frac{8\mathbf{i} - 5\mathbf{j} + 17\mathbf{k}}{3\sqrt{42}} \] Thus, the unit vector in the direction of \( \mathbf{CD} \) is: \[ \boxed{\frac{1}{\sqrt{42}}(8\mathbf{i} - 5\mathbf{j} + 17\mathbf{k})} \]
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.