# What is the ionic equation for magnesium and copper sulfate?

## What is the ionic equation for magnesium and copper sulfate?

The equation now reads: Cu2+ + Mg → Cu + Mg2+ This is called an ionic equation; it shows only the ions and atoms involved in the reaction.

### What happens when copper sulphate reacts with magnesium?

When magnesium is placed in copper sulfate solution a redox reaction occurs, causing copper metal to form on the magnesium and the deep blue colour of the solution pales. Therefore, it is possible to conclude that magnesium is more reactive than copper.

What does mg and CuSO4 make?

When you place a solid Mg ribbon into the blue CuSO4 solution, a metal displacement reaction occurs. The overall reaction is: Mg(s) + CuSO4(aq) –> MgSO4(aq) + Cu(s); the magnesium, because it is more reactive than copper, displaces it. The blue solution will turn reddish black with the introduction of Mg.

What is the ionic equation for magnesium?

Magnesium ion | Mg+2 – PubChem.

## Why is copper sulfate left for 4 minutes before adding the magnesium?

No reaction is seen if you do things the other way round – in other words, if you put copper powder into magnesium sulfate solution. This is because copper is not reactive enough to displace magnesium from magnesium sulfate.

### Does iron and magnesium sulfate react?

Solid iron and a solution of magnesium sulfate are made. This is called a displacement reaction. It happens because magnesium is more reactive than iron. The magnesium turns darker where it dips into the iron(II) sulfate solution and has become coated with iron.

Why was the highest rise in temperature obtained with magnesium and copper sulphate?

The magnesium will displace the copper and the temperature will rise. The Magnesium will displace the Copper and rise in temperature because it is more reactive and it is an exothermic reaction. The copper will be displaced because zinc is higher in the reactivity series than copper therefore zinc is more reactive.

Does magnesium react with ethanol?

If you are trying to prepare by reacting of magnesium metal with ethanol in the presence of some initiator like iodine then the reaction will start and will complete at higher temperature and if the moisture content is at higher side in the used ethanol then reaction will take more time for completion and if the …

## What happens when you add iron to copper sulphate?

Iron displaces copper ions from an aqueous solution of copper sulphate. In this reaction, metallic iron is converted into ferrous ion (Fe2+) and cupric ion (Cu2 +) is converted into metallic copper. Fe (s) + Cu2 + (aq) —→ Fe2+ (aq) + Cu (s).

### Is magnesium more reactive than zinc?

In a reactivity series, the most reactive element is placed at the top and the least reactive element at the bottom….The reactivity series.

Element Reaction with dilute acids
Magnesium Quickly
Zinc More slowly
Iron More slowly than zinc
Copper Very slowly

What is the chemical equation for magnesium and copper?

A balanced chemical equation. for the reaction between magnesium and copper(II) sulfate solution is: Mg(s) + CuSO 4 (aq) → MgSO 4 (aq) + Cu(s) It can be written using the ions involved:

What happens when you mix magnesium and copper sulphate?

The overall reaction is: Mg (s) + CuSO4 (aq) –> MgSO4 (aq) + Cu (s); the magnesium, because it is more reactive than copper, displaces it. The blue solution will turn reddish black with the introduction of Mg. What happens when you mix copper sulphate and magnesium?

## How to determine the reactivity of magnesium sulfate?

Determining a reactivity series Magnesium sulfate solution Copper (II) sulfate solution Iron (II) sulfate solution Number of reactions Magnesium Not done Brown coating Black coating 2 Copper No visible reaction Not done No visible reaction 0 Iron No visible reaction Brown coating Not done 1

### What happens when copper sulfate is in AQ state?

If the copper (II) SULFATE is in Aq state….. The blue coloration of the Cu 2+ ions will disappear and a colorless solution of magnesium sulfate will then form.