To find the electrostatic potential energy of the charge configuration, we can use the formula for the potential energy \( U \) between two point charges:
\(U = \frac{k \cdot q_1 \cdot q_2}{r}\)
where:
Given:
Now, calculate the electrostatic constant \( k \):
\(k = \frac{1}{4\pi\epsilon_0} = \frac{1}{4\pi \times 8.85 \times 10^{-12}} \approx 8.99 \times 10^9 \, \text{N m}^2 \text{C}^{-2}\)
Substitute all the values into the formula for \( U \):
\(U = \frac{8.99 \times 10^9 \times 7 \times 10^{-6} \times (-4) \times 10^{-6}}{0.14}\)
Calculate:
\(U = \frac{-8.99 \times 10^9 \times 28 \times 10^{-12}}{0.14}\)
\(U = \frac{-251.72 \times 10^{-3}}{0.14}\)
\(U = -1.8 \, \text{J}\)
Thus, the electrostatic potential energy of the charge configuration is \(-1.8 \, \text{J}\). Hence, the correct option is:
Answer: \( -1.8 \, \text{J} \)
For a short dipole placed at origin O, the dipole moment P is along the X-axis, as shown in the figure. If the electric potential and electric field at A are V and E respectively, then the correct combination of the electric potential and electric field, respectively, at point B on the Y-axis is given by:

An organic compound (X) with molecular formula $\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}$ is not readily oxidised. On reduction it gives $\left(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}(\mathrm{Y})\right.$ which reacts with HBr to give a bromide (Z) which is converted to Grignard reagent. This Grignard reagent on reaction with (X) followed by hydrolysis give 2,3-dimethylbutan-2-ol. Compounds (X), (Y) and (Z) respectively are: