The number of radial node/s for \(3 \mathrm{p}\) orbital is _______.

For the reaction \(\mathrm{A} \rightarrow \mathrm{B}\) the following graph was obtained. The time required (in seconds) for the concentration of A to reduce to \(2.5 \mathrm{~g} \mathrm{~L}^{-1}\) (if the initial concentration of A was \(50 \mathrm{~g} \mathrm{~L}^{-1}\)) is _______ (Nearest integer)
Given : \(\log 2=0.3010\) [We can assume in a hypothetical situation that the graph is correct, assuming its first order reaction, in reality the question is wrong.]

The reduction reaction known as:

\(IUPAC\) name of following compound \((\mathrm{P})\) is 

A compound with molecular mass \(180\) is acylated with \(CH_3COCl\) to get a compound with molecular mass \(390.\) The number of amino groups present per molecule of the former compound is :

The ' Spin only ' Magnetic moment for \(\left[\mathrm{Ni}\left(\mathrm{NH}_3\right)_6\right]^{2+}\) is _______ \(\times 10^{-1} \mathrm{BM}\). \((\) given \(=\) Atomic number of \(\mathrm{Ni}: 28)\)

The standard reduction potentials at \(298 \mathrm{~K}\) for the following half cells are given below : \(\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}+7 \mathrm{H}_2 \mathrm{O}, \mathrm{E}^{\circ}=1.33 \mathrm{~V}\) \(\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}  \mathrm{E}^{\circ}=-0.04 \mathrm{~V}\) \(\mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Ni}  \mathrm{E}^{\circ}=-0.25 \mathrm{~V}\) \(\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag} \mathrm{E}^{\circ}=0.80 \mathrm{~V}\) \(\mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Au} \mathrm{E}^{\circ}=1.40 \mathrm{~V}\) Consider the given electrochemical reactions, The number of metal\((s)\) which will be oxidized be \(\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}\), in aqueous solution is _______.

\(2 O _{3}( g ) \rightleftharpoons 3 O _{2}( g )\) At \(300 \,K\), ozone is fifty percent dissociated. The standard free energy change at this temperature and \(1\, atm\) pressure is \((-)\) \(........\,J\, mol ^{-1}\) (Nearest integer) [Given: \(\ln 1.35=0.3\) and \(R =8.3 J K ^{-1} mol ^{-1}\) ]

In the reported figure, there is a cyclic process \(ABCDA\) on a sample of \(1\, {mol}\) of a diatomic gas. The temperature of the gas during the process \({A} \rightarrow {B}\) and \({C} \rightarrow {D}\) are \({T}_{1}\) and \({T}_{2}\left({T}_{1}\,>\,{T}_{2}\right)\) respectively. Choose the correct option out of the following for work done if processes \(B C\) and \(D A\) are adiabatic.

The sum of all the elements in the range of \(f(x)=\text{Sgn}(\sin x)+\text{Sgn}(\cos x)+\text{Sgn}(\tan x)+\text{Sgn}(\cot x), x\ne\frac{n\pi}{2}, n\in Z\), where \(\operatorname{Sgn}(t)=\left\{\begin{array}{lll}1, & \text { if } & t>0 \\ -1 & \text { if } & t<0\end{array}\right.\), is

For electron in ' 2 s ' and ' 2 p ' orbitals, the orbital angular momentum values, respectively are :

The correct order of the spin only magnetic moment of metal ions in the following low spin complexes, \({\left[ {V\,{{\left( {CN} \right)}_6}} \right]^{4 - }}\) , \({\left[ {Fe\,{{\left( {CN} \right)}_6}} \right]^{4 - }}\) , \({\left[ {Ru\,{{\left( {N{H_3}} \right)}_6}} \right]^{3 + }}\) , and \({\left[ {Cr\,{{\left( {N{H_3}} \right)}_6}} \right]^{2 + }}\) , is

Given below are two statements :- Statement \(I:\)- In redox titration, the indicators used are sensitive to change in \(pH\) of the solution. Statement \(II:\)- In acid-base titration, the indicators used are sensitive to change in oxidation potential. In the light of the above statements, choose the most appropriate answer from the options given below