We are given that the angle between the lines joining the foci of an ellipse to one particular extremity of the minor axis is \( 90^\circ \). This condition is used to determine the eccentricity of the ellipse.
Step 1: Recall the geometry of an ellipse.
For an ellipse, the foci are located along the major axis, and the distance between the foci is \( 2c \), where \( c \) is the focal distance. The semi-major axis is \( a \), and the semi-minor axis is \( b \). The eccentricity \( e \) is
given by:
\[ e = \frac{c}{a}. \] The angle between the lines joining the foci to one particular extremity of the minor axis is related to the eccentricity \( e \).
Step 2: Use the condition on the angle.
The formula for the angle \( \theta \) between the lines joining the foci to the extremity of the minor axis is: \[ \tan \theta = \frac{2b}{\sqrt{a^2 - b^2}}. \] We are
given that \( \theta = 90^\circ \), so:
\[ \tan 90^\circ = \infty, \] which leads to the relationship: \[ \frac{2b}{\sqrt{a^2 - b^2}} = \infty. \] Solving this equation gives the eccentricity \( e = \frac{1}{\sqrt{3}} \). Thus, the correct answer is \( \frac{1{\sqrt{3}}} \).
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.