(a)
Interpretation:
The reaction of nitric oxide turns brown when exposed to air and its balanced equation has to be written.
Concept introduction:
Balanced Chemical equation:
A balanced chemical equation is an equation which contains same elements in same number on both the sides (reactant and product side) of the chemical equation thereby obeying the law of conservation of mass.
(b)
Interpretation:
The reaction of nitric acid turns yellow-brown on standing and its balanced equation has to be written.
Concept introduction:
Balanced Chemical equation:
A balanced chemical equation is an equation which contains same elements in same number on both the sides (reactant and product side) of the chemical equation thereby obeying the law of conservation of mass.
(c)
Interpretation:
Silver dissolves in dilute
Concept introduction:
Balanced Chemical equation:
A balanced chemical equation is an equation which contains same elements in same number on both the sides (reactant and product side) of the chemical equation thereby obeying the law of conservation of mass.
(d)
Interpretation:
The reaction of hydrazine reduces iodine to
Concept introduction:
Balanced Chemical equation:
A balanced chemical equation is an equation which contains same elements in same number on both the sides (reactant and product side) of the chemical equation thereby obeying the law of conservation of mass.
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General Chemistry: Atoms First
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- Complete and balance the following equations:(a) An active metal reacting with acid,Al(s)+HCl(aq)→ (b) A salt like (alkali metal) hydride reacting with water,LiH(s)+H2O(l)→arrow_forwardWrite a balanced net ionic equation for each of the followingreactions: (a) Dilute nitric acid reacts with zinc metalwith formation of nitrous oxide. (b) Concentrated nitricacid reacts with sulfur with formation of nitrogen dioxide.(c) Concentrated nitric acid oxidizes sulfur dioxide withformation of nitric oxide. (d) Hydrazine is burned in excessfluorine gas, forming NF3. (e) Hydrazine reduces CrO42- toCr(OH)4- in base (hydrazine is oxidized to N2).arrow_forward(a) Mention the optimum conditions for the industrial manufacture of ammonia by Haber’s process. (b) Explain the following giving appropriate reasons: (i) Sulphur vapour exhibits paramagnetic behaviour: (ii) Red phosphorus is less reactive than white phosphorusarrow_forward
- Write chemical equations for the following processes:(1) Reduction of VO2+to produce VO2+(2) Neutralization of sulfuric acid by barium hydroxide(3) Thermal decomposition of 1 mol of sodium bicarbonate to produce sodium carbonate,carbon dioxide and waterarrow_forwardWrite a balanced chemical equation for the reaction of an excess of oxygen with each of the following. Remember that oxygen is a strong oxidizing agent and tends to oxidize an element to its maximum oxidation state.(a) Mg(b) Rb(c) Ga(d) C2H2(e) COarrow_forward(a) A alkali metals react withhydrogen to form hydrides and react with halogens to formhalides. Compare the roles of hydrogen and halogens inthese reactions. Write balanced equations for the reaction offluorine with calcium and for the reaction of hydrogen withcalcium. (b) What is the oxidation number and electronconfiguration of calcium in each product?arrow_forward
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