Given four masses \( m \) are placed at the corners of a square with side \( a \). The net gravitational force on one mass due to the other three masses is given by:
\[ F_{\text{net}} = \sqrt{2}F + F' \]
Where:
\[ F = \frac{Gm^2}{a^2}, \quad F' = \frac{Gm^2}{(\sqrt{2}a)^2} \]
Substituting values:
\[ F_{\text{net}} = \sqrt{2}\frac{Gm^2}{a^2} + \frac{Gm^2}{2a^2} \]
Equating:
\[ \left( \frac{2\sqrt{2} + 1}{32} \right) \frac{Gm^2}{L^2} = \frac{Gm^2}{a^2} \left( \frac{2\sqrt{2} + 1}{2} \right) \]
Solving gives:
\[ a = 4L \]
37.8 g \( N_2O_5 \) was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K: \[ 2N_2O_5(g) \rightarrow 2N_2O_4(g) + O_2(g) \]
The total pressure at equilibrium was found to be 18.65 bar. Then, \( K_p \) is: Given: \[ R = 0.082 \, \text{bar L mol}^{-1} \, \text{K}^{-1} \]
The product (A) formed in the following reaction sequence is:
Which of the following statement is true with respect to H\(_2\)O, NH\(_3\) and CH\(_4\)?
(A) The central atoms of all the molecules are sp\(^3\) hybridized.
(B) The H–O–H, H–N–H and H–C–H angles in the above molecules are 104.5°, 107.5° and 109.5° respectively.
(C) The increasing order of dipole moment is CH\(_4\)<NH\(_3\)<H\(_2\)O.
(D) Both H\(_2\)O and NH\(_3\) are Lewis acids and CH\(_4\) is a Lewis base.
(E) A solution of NH\(_3\) in H\(_2\)O is basic. In this solution NH\(_3\) and H\(_2\)O act as Lowry-Bronsted acid and base respectively.
Quantitative analysis of an organic compound (X) shows the following percentage composition.
C: 14.5%
Cl: 64.46%
H: 1.8%
Empirical formula mass of the compound (X) is: