To solve this problem, we need to calculate the work done in rotating a bar magnet from its most stable position (parallel to the magnetic field) to its most unstable position (antiparallel to the magnetic field). The formula for the work done \( W \) in rotating a magnetic dipole in a magnetic field is given by:
where PE (Potential Energy) is calculated using:
Here, \( M \) is the magnetic moment, \( B \) is the magnetic field, and \( \theta \) is the angle with the magnetic field.
1. **Most Stable Position**: The magnetic dipole is aligned with the magnetic field. Therefore, \( \theta = 0^\circ \).
2. **Most Unstable Position**: The magnetic dipole is antiparallel to the magnetic field. Thus, \( \theta = 180^\circ \).
Substituting these into the formula for work done:
3. **Substitute Given Values**: \( M = 0.5 \, \text{Am}^2 \) and \( B = 8 \times 10^{-2} \, \text{T} \).
Therefore, the work done in rotating the magnet is \(\mathbf{8 \times 10^{-2} \, \text{J}}\).
The correct option is: \( \mathbf{8 \times 10^{-2} \, \text{J}} \).
Magnetic Potential Energy:
The potential energy U of a magnetic moment m in a uniform magnetic field B is given by:
U = -mB cos θ.
Stable and Unstable Equilibrium Positions:
1. At stable equilibrium (θ = 0°):
Ustable = -mB cos 0° = -mB.
2. At unstable equilibrium (θ = 180°):
Uunstable = -mB cos 180° = +mB.
Work Done:
The work done in rotating the magnet from the stable to the unstable position is the change in potential energy:
W = ΔU = Uunstable - Ustable = mB - (-mB) = 2mB.
Substitute Values:
Given:
m = 0.5 Am2, B = 8 × 10-2 T,
W = 2 × 0.5 × 8 × 10-2 = 8 × 10-2 J.
Answer: 8 × 10-2 J
A black body is at a temperature of 2880 K. The energy of radiation emitted by this body with wavelength between 499 nm and 500 nm is U1, between 999 nm and 1000 nm is U2 and between 1499 nm and 1500 nm is U3. The Wien's constant, b = 2.88×106 nm-K. Then,

What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)