The equation of the given circle \( x^2 + y^2 - 6|x| = 0 \) represents two circles, one with \( x \geq 0 \) and another with \( x < 0 \).
This equation can be rewritten as: \[ x^2 + y^2 = 6x \quad \text{for} \quad x \geq 0. \] Now, to find the equation of the circle that touches these two circles and has a radius of 3, we use the general formula for the equation of a circle: \[ (x - h)^2 + (y - k)^2 = r^2, \] where \( (h, k) \) is the center of the circle and \( r \) is its radius. By solving this geometrically or using the condition for tangency, we find that the correct equation is \( x^2 + y^2 + 6\sqrt{3}y + 18 = 0 \) or \( x^2 + y^2 - 6\sqrt{3}y + 18 = 0 \).
If the probability density function of a random variable is given by $$ f(x) = \begin{cases} 12x^2(1 - x), & 0 \leq x \leq 1 \\ 0, & \text{elsewhere} \end{cases} $$ then the mean and variance are respectively:
The area of a parallelogram whose diagonals are given by $ \vec{u} + \vec{v} $ and $ \vec{v} + \vec{w} $, where:
$ \vec{u} = 2\hat{i} - 3\hat{j} + \hat{k}, \quad \vec{v} = -\hat{i} + \hat{k}, \quad \vec{w} = 2\hat{j} - \hat{k} $ is:
The direction ratios of the normal to the plane passing through the points
$ (1, 2, -3), \quad (1, -2, 1) \quad \text{and parallel to the line} \quad \frac{x - 2}{2} = \frac{y + 1}{3} = \frac{z}{4} \text{ is:} $
At 15 atm pressure, $ \text{NH}_3(g) $ is being heated in a closed container from 27°C to 347°C and as a result, it partially dissociates following the equation: $ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) $ If the volume of the container remains constant and pressure increases to 50 atm, then calculate the percentage dissociation of $ \text{NH}_3(g) $
If equilibrium constant for the equation $ A_2 + B_2 \rightleftharpoons 2AB \quad \text{is} \, K_p, $ then find the equilibrium constant for the equation $ AB \rightleftharpoons \frac{1}{2} A_2 + \frac{1}{2} B_2. $
Consider the following reaction: $ \text{CO}(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) $ At 27°C, the standard entropy change of the process becomes -0.094 kJ/mol·K. Moreover, standard free energies for the formation of $ \text{CO}_2(g) $ and $ \text{CO}(g) $ are -394.4 and -137.2 kJ/mol, respectively. Predict the nature of the above chemical reaction.