Suggest a list of the substances where carbon can exhibit oxidation states from -4 to +4 and nitrogen from -3 to +5.
The substances where carbon can exhibit oxidation states from -4 to +4 are listed below:
Substance | Formula | Oxidation State of (C) |
Methan | CH4 | -4 |
Ethane | C2H6 | -3 |
Ethene | C2H4 | -2 |
Ethyne | C2H2 | -1 |
Dichloromethane | CH2Cl2 | 0 |
Chloroform | CHCl3 | +2 |
Oxalic Acid | (COOH)2 | +3 |
Carbon TetraChloride | CCl4 | +4 |
Carbon dioxide | CO2 | +4 |
The substances where nitrogen can exhibit oxidation states from -3 to +5 are listed below:
Substance | Formula | Oxidation State of Nitrogen |
Ammonia | NH3 | -3 |
Hydrazine | N2H4 | -2 |
Hydride | N2H2 | -1 |
Dinitrogen Gas | N2 | 0 |
Nitrous Oxide | N2O | +1 |
Nitric Oxide | NO | +2 |
Dinitrogen Trioxide | N2O3 | +3 |
Dinitrogen Dioxide | NO2 | +4 |
Nitrogen Pentroxide | N2O5 | +5 |
The mass of an electron is 9.1 × 10–31 kg. If its K.E. is 3.0 × 10–25 J, calculate its wavelength.
Calculate the amount of carbon dioxide that could be produced when
(i) 1 mole of carbon is burnt in air.
(ii) 1 mole of carbon is burnt in 16 g of dioxygen.
(iii) 2 moles of carbon are burnt in 16 g of dioxygen.
Calculate the wavelength of an electron moving with a velocity of 2.05 × 107 ms–1.
Balance the following redox reactions by ion – electron method :
(a) MnO4 – (aq) + I – (aq) → MnO2 (s) + I2(s) (in basic medium)
(b) MnO4 – (aq) + SO2 (g) → Mn2+ (aq) + HSO4– (aq) (in acidic solution)
(c) H2O2 (aq) + Fe 2+ (aq) → Fe3+ (aq) + H2O (l) (in acidic solution)
(d) Cr2O7 2– + SO2(g) → Cr3+ (aq) + SO42– (aq) (in acidic solution)
In a process, 701 J of heat is absorbed by a system and 394 J ofwork is done by the system. What is the change in internal energy for the process?
What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 at 30°C?
In a reaction A + B2 → AB2 Identify the limiting reagent, if any, in the following reaction mixtures.
(i) 300 atoms of A + 200 molecules of B
(ii) 2 mol A + 3 mol B
(iii) 100 atoms of A + 100 molecules of B
(iv) 5 mol A + 2.5 mol B
(v) 2.5 mol A + 5 mol B
At 0°C, the density of a certain oxide of a gas at 2 bar is same as that of dinitrogen at 5 bar. What is the molecular mass of the oxide?
Which one of the following will have largest number of atoms?
(i) 1 g Au (s)
(ii) 1 g Na (s)
(iii) 1 g Li (s)
(iv) 1 g of Cl2(g)
Density of a gas is found to be 5.46 g/dm3 at 27 °C at 2 bar pressure. What will be its density at STP?
Beryllium and magnesium do not give colour to flame whereas other alkaline earth metals do so. Why?
Suggest reasons why the B-F bond lengths in BF3 (130 pm) and BF-4(143 pm) differ.
Complete the following reactions:
Define the bond length.
What happens when
(a) Borax is heated strongly,
(b) Boric acid is added to water,
(c) Aluminium is treated with dilute NaOH,
(d) BF3 is reacted with ammonia?
Prefixes Multiples
(i) micro 106
(ii) deca 109
(iii) mega 10–6
(iv) giga 10–15
(v) femto 10
How can domestic waste be used as manure?
Write the significance of a plus and a minus sign shown in representing the orbitals.
Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2) with aqueous hydrochloric acid according to the reaction
4HCl(aq) + MnO2(s) → 2H2O(l) + MnCl2(aq) + Cl2(g)
How many grams of HCl react with 5.0 g of manganese dioxide?
What is Kc for the following equilibrium when the equilibrium concentration of each substance is: [SO2]= 0.60 M, [O2] = 0.82 M and [SO3] = 1.90 M ?
2SO2(g) + O2(g) ↔ 2SO3(g)