Class 10 Chemical equations and reaction Test Paper
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Short Answer Questions
Question 1. what is the ratio of number of moles of reactants to the number of moles of products in the equation.
H2S (g) + SO2 (g) -> S (s) + H2O (liq) Solution
2H2S (g) + SO2 (g) -> 3S (s) + 2H2O (liq)
Ratio of number of moles of reactants to the number of moles of products= 3/5
Question 2. In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the reaction involves. Solution
When copper is mixed in silver nitrate solution, it displaces the silver because copper is more reactive than silver.
2AgNO3 + Cu —> Cu(NO3)2 + 2Ag
Question 3.Translate the following statements into chemical equations and then balance them.
a)Hydrogen gas combines with nitrogen to form ammonia
b)Hydrogen sulphide gas burns in air to give water and sulfur dioxide.
c)Barium chloride reacts with aluminum sulphate to give aluminum chloride and a precipitate of barium sulphate.
d)Potassium metal reacts with water to give potassium hydroxide and hydrogen gas. Solution
Question 5.Why is respiration considered as an exothermic reaction? Explain. Question 6.What is rancidity? Question 7.Write the balanced chemical equation of the following and identify the type of reaction in each case:
i.Potassium bromide (aq) + Barium iodide (s)
ii.Zinc carbonate (s) -> Zinc oxide (s) + Carbon dioxide (g)
iii.Magnesium (s) + hydrochloric acid (aq)->Magnesium chloride (aq) + Hydrogen (g) Solution
Question 9.Balance the chemical equations for the following important industrial processes:
a)Molecular nitrogen and hydrogen combine to give ammonia.
b)Molecular hydrogen and carbon monoxide react to form methanol (CH3OH).
c)CaO + C ->CO + CaC2
d)C2H4 + O2+ HCl -> C2H4Cl2 + H2O Solution
a) N2 + 3H2 -> NH3
b) 4H2 + 2CO -> 2CH3OH
c) CaO + 3C ->CO + CaC2
d) 2C2H4 + O2 + 4HCl -> 2C2H4Cl2 + 2H2O
Question 12.Represent each of the following word equations with a balanced chemical equation.
a)Disilane gas (Si2H6) undergoes combustion to form solid silicon dioxide and water.
b)Solid aluminum hydride is formed by a combination reaction of its two elements.
c)When solid calcium bi sulfate is heated, it decomposes to solid calcium oxide, sulfur dioxide gas, and water. Question 13.A large piece of zinc metal is placed in a copper (II) sulfate, CuSO4, solution. The blue solution become colorless as copper metals falls to the bottom of the container. The resulting solution contains zinc sulfate, ZnSO4. Write balanced formula unit, total ionic, and net ionic equations for the reaction Question 14.A solution of AgNO3 is mixed with a solution of K2S. write the molecular, total ionic and net ionic equations illustrating the reaction. Question 15.Write decomposition reactions for the following compounds
a)Ca(HCO3)2
b)Ag2O
c)N2O3 Question 16.Write one equation each for decompositions reactions where energy is supplied in the form of heat, light or electricity. Solution
When Calcium Carbonate is heated, it decomposes to give calcium oxide and carbon dioxide :-
CaCO3 (s) -----Heat----> CaO (s) + CO2
When electric current is passed through H2O, it decomposes to give $H_2$ and $O_2$:-
2H2O (l) ----Electricity----> 2H2 (g) + O2 (g)
When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas:-
2AgCl (s) ----Light----> 2Ag (s) + Cl2 (g)
Long Answer Questions
Question 1.What do you understand by exothermic and endothermic reactions? Explain with one example each? Write a balanced chemical equation for the process of photosynthesis and the condition of the reaction giving physical state of all the substances? Question 2.Why decomposition reactions are called the opposite of combination reactions? Write equations for these reactions. Discuss the importance of decomposition reaction in metal industries with three points? Question 3.What do you mean by precipitation reactions? Explain by giving examples. Question 4.Illustrate an activity to show a double displacement reaction. Give the chemical equation of the reaction that takes place. Write the physical state of the product obtained? Question 5.Balance the following equations
(i)KClO3 -> KCl + O2
(ii)H2SO4 + NaOH -> Na2SO4 + H2O
(iii)H2O2 -> H2O + O2
(iv)Na2CO3 + HCl -> NaCl + NaHCO3
(v)Mg + N2 -> Mg3N2
(vi)Fe + H2O -> Fe3O4 +H2
(vii)MnO2 + Al -> Mn + Al2O3
(viii)Si2H6 + H2O -> Si(OH)4 + H2
(ix)NH3 + O2 -> NO + H2O
(x)B4H10 + O2 -> B2O3 + H2O
(xi)Al + CuCl2 -> AlCl3 + Cu Solution
Question 6.The oxidation of iron to rust is a problem, but the oxidation of aluminum to aluminum oxide is not why? Question 7.Write balanced equations by predicting the products of the following reactions. Include the physical state of each element or compound.
a)Phosphorus burn in chlorine to form phosphorus pentachloride.
b)A single- displacement reaction of calcium metal with a nitric acid solution
c)Burning of natural gas.
d)The process of respiration.
e)When a green iron salt is heated strongly, its color finally changes to black and odor of burning sulfur is given out.
