List of top Chemistry Questions

Consider the reactions:
\(2S_2O_3^{2-}(aq) + I_2(s) \rightarrow S_4O_6^{2-}(aq) + 2I ^- (aq)\)
\(S_2O_3^{2-}(aq) + 2Br_2(l) + 5 H_2O(l) \rightarrow 2SO_4^{2-}(aq) + 4Br ^- (aq) + 10H ^+ (aq)\) 
Why does the same reductant, thiosulphate react differently with iodine and bromine?

What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? (For iron sulphide, Ksp = 6.3 × 10^–18).

How do you count for the following observations?

1. Though alkaline potassium permanganate and acidic potassium permanganate both are used as oxidants, yet in the manufacture of benzoic acid from toluene we use alcoholic potassium permanganate as an oxidant. Why? Write a balanced redox equation for the reaction.
2. When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smelling gas HCl, but if the mixture contains bromide then we get red vapour of bromine. Why?

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed. Will it lead to the precipitation of copper iodate? (For cupric iodate K_sp = 7.4 × 10^–8).

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

Electromagnetic radiation of wavelength 242 nm is just sufficient to ionize the sodium atom. Calculate the ionization energy of sodium in kJ mol^–1.

What sorts of information can you draw from the following reaction?
(CN)_2(g)+2OH^-_(aq)\(\rightarrow\)CN^-_(aq)+CNO^-_(aq)+H₂O_(l)

A photon of wavelength \(4×10^{–7} m\) strikes on metal surface, the work function of the metal being \(2.13\ eV\). Calculate:

1. the energy of the photon (eV)
2. the kinetic energy of the emission, and
3. the velocity of the photo electron (\(1\ eV= 1.6020×10^{–19} J\)).

Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298K from their solubility product constants.Determine also the molarities of individual ions.

Consider the elements: \(Cs\), \(Ne\), \(I\) and \(F\)

1. Identify the element that exhibits only negative oxidation state. 
2. Identify the element that exhibits only postive oxidation state. 
3. Identify the element that exhibits both positive and negative oxidation states.
4. Identify the element which exhibits neither the negative nor does the positive oxidation state.

Refer to the periodic table given in your book and now answer the following questions:

1. Select the possible non metals that can show disproportionation reaction. 
2. Select three metals that can show disproportionation reaction

Predict the products of electrolysis in each of the following:

1. An aqueous solution of \(AgNO_3\) with silver electrodes
2. An aqueous solution \(AgNO_3\) with platinum electrodes 
3. A dilute solution of \(H_2SO_4\) with platinum electrodes 
4. An aqueous solution of \(CuCl_2\) with platinum electrodes.

Calculate the wavelength, frequency and wave number of a light wave whose period is \(2.0×10^{–10}\ s\).

What is the number of photons of light with a wavelength of 4000 pm that provide 1J of energy?

Arrange the following metals in the order in which they displace each other from the solution of their salts.
Al, Cu, Fe, Mg and Zn.

Calculate the pH of the resultant mixtures: 
a) 10 mL of 0.2M Ca(OH)₂ + 25 mL of 0.1M HCl 
b) 10 mL of 0.01M H₂SO₄ + 10 mL of 0.01M Ca(OH)₂
c) 10 mL of 0.1M H₂SO₄ + 10 mL of 0.1M KOH

The ionic product of water at 310 K is 2.7 × 10^–14. What is the pH of neutral water at this temperature?

Given the standard electrode potentials,
K⁺ /K = -2.93V,
Ag⁺/Ag = 0.80V, 
Hg²⁺/Hg = 0.79V 
Mg²⁺/Mg = -2.37V.
Cr³⁺/Cr = -0.74V
Arrange these metals in their increasing order of reducing power.

Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺ (aq) \(\rightarrow\)  Zn²⁺ (aq) + 2Ag(s) takes place, further show: 

1. which of the electrode is negatively charged, 
2. the carriers of the current in the cell, and
3. individual reaction at each electrode.

Write IUPAC names of the following compounds:

Fluorine reacts with ice and results in the change:
\(H_2O(s) + F_2{(g)} \rightarrow HF{(g)} + HOF{(g)}\) Justify that this reaction is a redox reaction.

While sulphur dioxide and hydrogen peroxide can act as oxidising as well as reducing agents in their reactions, ozone and nitric acid act only as oxidants. Why?

Suggest a list of the substances where carbon can exhibit oxidation states from -4 to +4 and nitrogen from -3 to +5.

Write the formulae for the following compounds: 
(a) Mercury (II) chloride (b) Nickel (II) sulphate 
(c) Tin (IV) oxide (d) Thallium (I) sulphate 
(e) Iron (III) sulphate (f) Chromium (III) oxide

The ionization constant of chloroacetic acid is 1.35 × 10^–3. What will be the pH of 0.1M acid and its 0.1M sodium salt solution?