For a hollow sphere rolling on a plane surface, the total kinetic energy \( K_{\text{total}} \) consists of translational kinetic energy \( K_{\text{trans}} \) and rotational kinetic energy \( K_{\text{rot}} \).
Step 1: Expressions for Kinetic Energy
The translational kinetic energy is given by:
\[ K_{\text{trans}} = \frac{1}{2} mv^2, \]
where \( m \) is the mass and \( v \) is the linear velocity of the center of mass.
The rotational kinetic energy about the axis of symmetry is given by:
\[ K_{\text{rot}} = \frac{1}{2} I \omega^2, \]
where \( I \) is the moment of inertia and \( \omega \) is the angular velocity.
For a hollow sphere:
\[ I = \frac{2}{3} m R^2, \]
where \( R \) is the radius of the sphere.
Step 2: Relating Translational and Rotational Motion
Since the sphere rolls without slipping:
\[ v = R \omega. \]
Step 3: Substituting the Moment of Inertia
The rotational kinetic energy becomes:
\[ K_{\text{rot}} = \frac{1}{2} \left( \frac{2}{3} m R^2 \right) \omega^2 = \frac{1}{3} m R^2 \omega^2. \]
Using \( v = R \omega \):
\[ K_{\text{rot}} = \frac{1}{3} m v^2. \]
Step 4: Calculating the Total Kinetic Energy
The total kinetic energy is:
\[ K_{\text{total}} = K_{\text{trans}} + K_{\text{rot}} = \frac{1}{2} m v^2 + \frac{1}{3} m v^2. \]
Combining terms:
\[ K_{\text{total}} = \frac{5}{6} m v^2. \]
Step 5: Finding the Ratio of Kinetic Energies
The ratio of rotational kinetic energy to total kinetic energy is:
\[ \text{Ratio} = \frac{K_{\text{rot}}}{K_{\text{total}}} = \frac{\frac{1}{3} m v^2}{\frac{5}{6} m v^2} = \frac{2}{5}. \]
Thus:
\[ \frac{x}{5} = \frac{2}{5} \implies x = 2. \]
Therefore, the value of \( x \) is 2.
Let \[ I(x) = \int \frac{dx}{(x-11)^{\frac{11}{13}} (x+15)^{\frac{15}{13}}} \] If \[ I(37) - I(24) = \frac{1}{4} \left( b^{\frac{1}{13}} - c^{\frac{1}{13}} \right) \] where \( b, c \in \mathbb{N} \), then \[ 3(b + c) \] is equal to:
For the thermal decomposition of \( N_2O_5(g) \) at constant volume, the following table can be formed, for the reaction mentioned below: \[ 2 N_2O_5(g) \rightarrow 2 N_2O_4(g) + O_2(g) \] Given: Rate constant for the reaction is \( 4.606 \times 10^{-2} \text{ s}^{-1} \).