Displacement Reactions
Chemistry ⇒ Chemical Reactions and Equations
Displacement Reactions starts at 9 and continues till grade 12.
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See sample questions for grade 9
A student adds a strip of zinc metal to a solution of copper(II) sulfate. What will be observed?
A student adds iron nails to a solution of copper(II) sulfate. After some time, the blue color of the solution fades and a reddish-brown deposit forms. What type of reaction is this?
A student adds magnesium ribbon to a solution of iron(II) sulfate. What will be the products of the reaction?
A student observes that when a piece of magnesium is added to copper(II) sulfate solution, the blue color fades and a reddish-brown solid forms. What is the identity of the solid?
Describe the difference between a single displacement and a double displacement reaction.
Describe what happens when a piece of copper is placed in a solution of silver nitrate.
Explain why a displacement reaction does not occur when copper is added to zinc sulfate solution.
Explain why chlorine can displace bromine from potassium bromide but not from sodium chloride.
Explain why magnesium can displace zinc from zinc sulfate solution but copper cannot.
Explain why potassium reacts vigorously with water, while copper does not.
Explain why sodium cannot be displaced from sodium chloride by any other metal.
Write a balanced chemical equation for the reaction between iron and copper(II) sulfate.
Write the balanced chemical equation for the reaction between chlorine gas and potassium iodide solution.
A solution contains both copper(II) sulfate and silver nitrate. If a piece of zinc is added, which metals will be deposited and why?
A student places a strip of lead metal into a solution of copper(II) nitrate. Predict whether a displacement reaction will occur and justify your answer using the reactivity series.
Arrange the following metals in order of decreasing ability to displace hydrogen from acids: magnesium, iron, silver, zinc.
Explain, with a balanced chemical equation, why aluminium can displace iron from iron(III) oxide but not from magnesium oxide.
Write a balanced chemical equation for the reaction that occurs when chlorine gas is bubbled through a solution of sodium iodide.
A solution contains both iron(II) sulfate and copper(II) sulfate. If a piece of magnesium is added, which metals will be deposited and why?
A student adds a strip of copper to a solution of iron(II) sulfate and observes no visible change. What does this indicate about the relative reactivity of copper and iron?
