Which of the following reagents can be used to convert Ethanol to Ethanal?
(A) Chromium trioxide in Pyridine and HCI
(B) Heated Copper at 573 K
(C) Anhydrous Chromium trioxide
(D) Acidic KMnO\(_4\)
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What is the oxidation state of Pt in \(\left( PtF _5\right)_4\) ?

A first order reaction is found to have rate constant \(k=3.0 \times 10^{-1} \mathrm{~s}^{-1}\). The half-life of the reaction will be:

Glucose gets oxidised to gluconic acid on reaction with bromine water. This indicates the presence of :

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When a metal is placed in a solution of its ions, the metal can lose electron and can go in the solution as ion or the metal ion in the solution can take electron from the electrode and get deposited as metal. Thus, the electrode acquires either positive or negative charge with respect to the solution leading to the development of a potential difference between the metal electrode and the solution. This potential difference is called the electrode potential of the metal. The electrode potential of a metal is a measure of relative tendency to undergo oxidation (loss of electron) or reduction (gain of electron). When the concentration of the ions in the solution is unity, the electrode potential is called standard electrode potential. The magni of potential depends upon the nature of electrode, concentration of ions in solution and the temperature. In a galvanic cell, the electrode at which oxidation occurs is known as anodic half-cell and the electrode at which reduction occurs is known as cathodic half cell. The emf of the cell in terms of standard reduction potential is given by \(E_{\text {cell }}^{\circ}=E_{\text {cathode }}^{\circ}-E_{\text {anode. }}^{\circ}\).The standard free energy change of the redox reaction taking place in the cell is related to \(E_{\text {cell }}^{\circ}\) by \(\Delta G^{\circ}=-n F E^{\circ}\). A redox reaction would occur spontaneously if the free energy change is negative. The equilibrium constant of the reaction is related to the standard free energy change by \(\Delta G^{\circ}=-R T \ln K\).
The equillibrium constant of a feasible cell reaction is

The solute and solvent in "Amalgam of mercury with sodium" are

For the reaction: \(2 A_2(g)+1 / 4 X ( g ) \rightarrow 2 A_2 X ( g )\), if the volume is increased to double its value by decreasing the pressure, and the reaction is first order with respect to \(X\) and second order with respect to \(A _2\), the rate of reaction will:

If \(A=\left[\begin{array}{ccc}-1 & 2 & 3 x \\ 2 y & 4 & -1 \\ 6 & -1 & 0\end{array}\right]\) is a symmetric matrix, then the value of 22 - y is:

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Alcohols are versatile compounds as they can act as both nucleophile and electrophile. They undergo reactions based on cleavage of O-H and C-O bonds. The cleavage of O-H bond reflects the acidic character of alcohols. However they are weaker acids than water, phenol and carboxylic acids. Alkoxide ion formed by loss of proton from the OH group of alcohols reacts with water to form the corresponding conjugate acid - base pair. They act as Bronsted base due to presence of unshared electron pairs on oxygen.Both alcohols and phenol react with carboxylic acids, acid chlorides and anhydrides to form esters. The introduction of acetyl group in alcohols or phenol is known as acetylation. Alcohols react with hydrogen halides to form alkyl halides which form the basis of Lucas test. They also undergo acid catalyzed dehydration to form alkenes. Alcohols can be easily oxidized with variety of oxidizing agents. The nature of the product depends on the type of oxidizing agent and the nature of alcohol.
Pyridinium chlorochromate is used for:

If \(a+b+c=\pi\), then the value of \(\left|\begin{array}{ccc}\sin (a+b+c) & \sin (a+c) & \cos b \\ -\sin b & 0 & \tan a \\ \cos (a+c) & \tan (b+c) & 0\end{array}\right|\) is:

Which reagent will distinguish Benzophenone from acetone ?

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A homogeneous mixture of two or more than two components has uniform composition and properties. The binary solutions have two components, which may be solid, liquid or gas. The resultant solution has a larger amount of solvent and a smaller amount of solute. The amount of solute in a given amount of solvent decides the concentration of the resulting solution. The concentration can be expressed in various ways, like molarity, molality, normality and mole fraction.
Glucose dissolved in water and ethanol dissolved in water are examples of:

Match List - I with List - II.

List - I (Pathogen)	List - II (Disease)
(A) Wuchereria	(I) Typhoid
(B) Plasmodium	(II) Pneumonia
(C) Streptococcus	(III) Malaria
(D) Salmonella	(IV) Elephantiasis

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