Consider the below reaction, and choose the correct statement:

In Dumas' method 292 mg of an organic compound released 50 mL of nitrogen gas \(\left(\mathrm{N}_2\right)\) at 300 K temperature and 715 mm Hg pressure. The percentage composition of ' N ' in the organic compound is ________ % (Nearest integer)
(Aqueous tension at \(300 \mathrm{~K}=15 \mathrm{~mm} \mathrm{Hg}\))

When a small amount of \(KMnO_4\) is added to concentrated \(H_2SO_4\), a green oily compound is obtained which is highly explosive in nature. Compound may be

The number of interhalogens from the following having square pyramidal structure is. \(ClF _{3}, IF _{7}, BrF _{5}, BrF _{3}, I _{2} Cl _{6}, IF _{5}, ClF , ClF _{5}\)

Match List \(I\) with List \(II\):

List \(I\) (Complexes)	List \(II\) (Hybridisation)
\(A\) \(\left[ Ni ( CO )_4\right]\)	\(I\) \(sp ^3\)
\(B\) \(\left[ Cu \left( NH _3\right)_4\right]^{2+}\)	\(II\) \(dsp^2\)
\(C\) \(\left[ Fe \left( NH _3\right)_6\right]^{2+}\)	\(III\) \(sp^3d^2\)
\(D\) \(\left[ Fe \left( H _2 O \right)_6\right]^{2+}\)	\(IV\) \(d^2sp^3\)

The bond dissociation enthalpy of \(\mathrm{X}_2 \Delta \mathrm{H}_{\text {bond }}\) calculated from the given data is _______ \(\mathrm{kJ} \mathrm{mol}^{-1}\). (Nearest integer)
\(\begin{aligned}
& \mathrm{M}^{+} \mathrm{X}^{-}(\mathrm{s}) \rightarrow \mathrm{M}^{+}(\mathrm{g})+\mathrm{X}^{-}(\mathrm{g}) \Delta \mathrm{H}_{\text {lattice }}^*=800 \mathrm{~kJ} \mathrm{~mol}^{-1} \\
& \mathrm{M}(\mathrm{~s}) \rightarrow \mathrm{M}(\mathrm{~g}) \Delta \mathrm{H}_{\text {sub }}^{\circ}=100 \mathrm{~kJ} \mathrm{~mol}^{-1}
\end{aligned}\)
\(\mathrm{M}(\mathrm{~g}) \rightarrow \mathrm{M}^{+}(\mathrm{g})+\mathrm{e}^{-}(\mathrm{g}) \Delta \mathrm{H}_{\mathrm{i}}=500 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
\(\mathrm{X}(\mathrm{~g})+\mathrm{e}^{-}(\mathrm{g}) \rightarrow \mathrm{X}^{-}(\mathrm{g}) \Delta \mathrm{H}_{\mathrm{eg}}^*=-300 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
\(\mathrm{M}(\mathrm{~s})+\frac{1}{2} \mathrm{X}_2(\mathrm{~g}) \rightarrow \mathrm{M}^{+} \mathrm{X}^{-}(\mathrm{s}) \Delta \mathrm{H}_f^{\circ}=-400 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
[Given : \(\mathrm{M}^{+} \mathrm{X}^{-}\)is a pure ionic compound and X forms a diatomic molecule \(\mathrm{X}_2\) in gaseous state]

Consider the following reaction, the rate expression of which is given below \(\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}\) \(\text { rate }=\mathrm{k}[\mathrm{A}]^{1 / 2}[\mathrm{~B}]^{1 / 2}\) The reaction is initiated by taking \(1 \mathrm{M}\) concentration \(A\) and \(B\) each. If the rate constant \((k)\) is \(4.6 \times 10^{-2} \mathrm{~s}^{-1}\), then the time taken for \(\mathrm{A}\) to become \(0.1 \mathrm{M}\) is _______ sec. (nearest integer)

The output of the given circuit diagram is _______.

A satellite of mass \(\frac{M}{2}\) is revolving around earth in a circular orbit at a height of \(\frac{R}{3}\) from earth surface. The angular momentum of the satellite is \(M \sqrt{\frac{G M R}{x}}\). The value of \(x\) is ______ , where \(M\) and \(R\) are the mass and radius of earth, respectively. ( G is the gravitational constant)

The bond order and the magnetic characteristics of \(CN^-\) are

Let \(f : R \rightarrow R\) be a differentiable function such that \(f \left(\frac{\pi}{4}\right)=\sqrt{2}, f \left(\frac{\pi}{2}\right)=0\) and \(f ^{\prime}\left(\frac{\pi}{2}\right)=1\) and let \(g(x)=\int\limits_{x}^{\pi / 4}\left(f^{\prime}(t) \sec t+\tan t \operatorname{sectf}(t)\right) d t\) for \(x \in\left[\frac{\pi}{4}, \frac{\pi}{2}\right)\). Then \(\lim\limits _{ x \rightarrow\left(\frac{\pi}{2}\right)^{-}} g ( x )\) is equal to

The eccentricity of an ellipse whose centre is at the origin is \(\frac{1}{2}\) . If one of its directices is \(x = - 4\) then the equation of the normal to it at \(\left( {1,\frac{3}{2}} \right)\) is

' \(X\) ' is the number of electrons in \(t_{2 g}\) orbitals of the most stable complex ion among \(\left[\mathrm{Fe}\left(\mathrm{NH}_3\right)_6\right]^{3+}\), \(\left[\mathrm{Fe}\left(\mathrm{Cl}_6\right)\right]^{3-},\left[\mathrm{Fe}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]^{3-}\) and \(\left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{3+}\). The nature of oxide of vanadium of the type \(\mathrm{V}_2 \mathrm{O}_{\mathrm{X}}\) is _______.