you are given the following materials Marble chips Dilute hydrochloric acid Zinc granules Identify the type of reaction when marble chips and zinc granules are added separately to acid taken in two tubes. Write chemical equations
CaCO3(s) + 2HCl (aq) ———–> CaCl2(aq) + H2CO3(aq) (CO2+H2O) II) Zn(S) + 2HCl(aq) ———–> ZnCl2(aq) + H2(g)
Write balanced equation for the reaction between magnesium and hydrochloric acid. Name the product obtained, identify the type of reaction.
The product formed is magnesium chloride and hydrogen gas. It is a displacement reaction.
Which products will be obtained when lead nitrate is heated simply. State the type of chemical reaction that occur in the change.
Lead monoxide, nitrogen dioxide and oxygen gas will be liberated. ii) Decomposition
What is observed when a solution of potassium iodide solution is added to a solution of lead nitrate? Name the type of reaction. Write a balanced chemical equation to represent the above chemical reaction.
Yellow precipitate of lead iodide is formed. It is precipitation reaction. Pb( NO3)2 (aq) + 2KI (aq) —-> Pbl2 (s) + 2KNO3 (aq) It is also called double displace
2g of ferrous sulphate crystals are heated in a dry boiling tube. (i) List any two observations. (ii) Name the type of chemical reaction taking place.
reen colour of Fe SO4 disappears and reddish brown solid is formed. • Smell of burning sulphur. (ii) Decomposition reaction chemical-reactions-and-equations-cha
Define a balanced chemical equation.
Balanced chemical equation has an equal number of atoms of different elements in the reactants and products.
We need to balance a skeltal chemical equation.” Give reason to justify the statement.
We need to balance chemical equation because of law of conservation of mass. It states that ‘matter can neither be created nor be destroyed’. Therefore chemical
State the type of chemical reactions and chemical equations that take place in the following: (i) Magnesium wire is burnt in air.
2MG+o2---> 2MgO
Write any two observation of this reaction
Exothermic and combination reaction, formation of Ca(OH)2