Displacement Reactions Involving Metals and Non-metals
Chemistry ⇒ Metals and Non-metals
Displacement Reactions Involving Metals and Non-metals starts at 8 and continues till grade 12.
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See sample questions for grade 12
A piece of silver is placed in a solution of copper(II) nitrate. Will a reaction occur? Justify your answer.
A solution contains both copper(II) sulfate and silver nitrate. If a piece of zinc is added, which metals will be displaced?
A strip of magnesium is placed in a solution of copper(II) sulfate. What will you observe?
A student adds a strip of copper to a solution of zinc sulfate. Will a reaction occur? Explain your answer.
A student adds bromine water to a solution of potassium chloride. Will a displacement reaction occur? Explain.
Arrange the following metals in order of decreasing reactivity based on their ability to displace others from salt solutions: Iron, Zinc, Copper, Magnesium.
Calculate the mass of copper deposited when 6.5 g of zinc reacts completely with excess copper(II) sulfate solution. (Zn = 65, Cu = 63.5)
Calculate the number of moles of hydrogen gas produced when 2 g of magnesium reacts with excess hydrochloric acid. (Mg = 24)
Describe the changes in oxidation states for the elements involved in the reaction: Fe + CuSO4 → FeSO4 + Cu.
Describe the role of the reactivity series in predicting displacement reactions.
Describe what happens when a piece of iron is placed in a solution of silver nitrate.
Explain why displacement reactions are considered redox reactions.
Explain why gold does not take part in displacement reactions with other metal salts.
Explain why hydrogen is included in the reactivity series of metals.
Explain why sodium cannot be displaced from its compounds by any other metal.
In the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s), which element is reduced?
Write the balanced chemical equation for the reaction between chlorine gas and potassium iodide solution.
