Reactivity 3.2.8—An electrolytic cell is an electrochemical cell that converts electrical energy to chemical energy by bringing about non-spontaneous reactions. Explain how current is conducted in an electrolytic cell. Deduce the products of the electrolysis of a molten salt.

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Which product will be obtained at the anode (positive electrode) when molten NaCl is electrolysed?

A. Na (l)

B. Cl (g)

C. Cl₂ (g)

D. Na (s)

Consider the following electrochemical cell.

What happens to the ions in the salt bridge when a current flows?

A. Na⁺ ions flow to the zinc half-cell and SO₄²⁻ ions flow to the copper half-cell.

B. Na⁺ ions flow to the copper half-cell and SO₄²⁻ ions flow to the zinc half-cell.

C. Na⁺ and SO₄²⁻ ions flow to the copper half-cell.

D. Na⁺ and SO₄²⁻ ions flow to the zinc half-cell.

Consider the following electrochemical cell.

What happens to the ions in the salt bridge when a current flows?

A. Na⁺ ions flow to the zinc half-cell and SO₄²⁻ ions flow to the copper half-cell.

B. Na⁺ ions flow to the copper half-cell and SO₄²⁻ ions flow to the zinc half-cell.

C. Na⁺ and SO₄²⁻ ions flow to the copper half-cell.

D. Na⁺ and SO₄²⁻ ions flow to the zinc half-cell.

Consider the following electrochemical cell.

What happens to the ions in the salt bridge when a current flows?

A. Na⁺ ions flow to the zinc half-cell and SO₄²⁻ ions flow to the copper half-cell.

B. Na⁺ ions flow to the copper half-cell and SO₄²⁻ ions flow to the zinc half-cell.

C. Na⁺ and SO₄²⁻ ions flow to the copper half-cell.

D. Na⁺ and SO₄²⁻ ions flow to the zinc half-cell.

Consider the following electrochemical cell.

What happens to the ions in the salt bridge when a current flows?

A. Na⁺ ions flow to the zinc half-cell and SO₄²⁻ ions flow to the copper half-cell.

B. Na⁺ ions flow to the copper half-cell and SO₄²⁻ ions flow to the zinc half-cell.

C. Na⁺ and SO₄²⁻ ions flow to the copper half-cell.

D. Na⁺ and SO₄²⁻ ions flow to the zinc half-cell.

Pure magnesium needed for making alloys can be obtained by electrolysis of molten magnesium chloride.

© International Baccalaureate Organization 2020.

Write the half-equations for the reactions occurring in this electrolysis.

Pure magnesium needed for making alloys can be obtained by electrolysis of molten magnesium chloride.

© International Baccalaureate Organization 2020.

Write the half-equations for the reactions occurring in this electrolysis.

Which statements are correct for electrolysis?

I.   An exothermic reaction occurs.
II.  Oxidation occurs at the anode (positive electrode).
III. The reaction is non-spontaneous.

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which statements are correct for electrolysis?

I.   An exothermic reaction occurs.
II.  Oxidation occurs at the anode (positive electrode).
III. The reaction is non-spontaneous.

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which statements are correct for electrolysis?

I.   An exothermic reaction occurs.
II.  Oxidation occurs at the anode (positive electrode).
III. The reaction is non-spontaneous.

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which statements are correct for electrolysis?

I.   An exothermic reaction occurs.
II.  Oxidation occurs at the anode (positive electrode).
III. The reaction is non-spontaneous.

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

What are the products of the electrolysis of molten potassium chloride, $\text{KCl\hspace{0.05em}(l)}$?

What are the products of the electrolysis of molten potassium chloride, $\text{KCl\hspace{0.05em}(l)}$?

What are the products of the electrolysis of molten potassium chloride, $\text{KCl\hspace{0.05em}(l)}$?

What are the products of the electrolysis of molten potassium chloride, $\text{KCl\hspace{0.05em}(l)}$?

Which statement is correct about the electrolysis of molten lead(II) bromide, PbBr₂?

A.  Br⁻ ions accept electrons at the cathode (negative electrode).

B.  Pb²⁺ ions accept electrons at the anode (positive electrode).

C.  Br⁻ ions lose electrons at the anode (positive electrode).

D.  Pb²⁺ ions lose electrons at the cathode (negative electrode).

Which statement is correct about the electrolysis of molten lead(II) bromide, PbBr₂?

A.  Br⁻ ions accept electrons at the cathode (negative electrode).

B.  Pb²⁺ ions accept electrons at the anode (positive electrode).

C.  Br⁻ ions lose electrons at the anode (positive electrode).

D.  Pb²⁺ ions lose electrons at the cathode (negative electrode).

Which statement is correct about the electrolysis of molten lead(II) bromide, PbBr₂?

A.  Br⁻ ions accept electrons at the cathode (negative electrode).

B.  Pb²⁺ ions accept electrons at the anode (positive electrode).

C.  Br⁻ ions lose electrons at the anode (positive electrode).

D.  Pb²⁺ ions lose electrons at the cathode (negative electrode).

Which statement is correct about the electrolysis of molten lead(II) bromide, PbBr₂?

A.  Br⁻ ions accept electrons at the cathode (negative electrode).

B.  Pb²⁺ ions accept electrons at the anode (positive electrode).

C.  Br⁻ ions lose electrons at the anode (positive electrode).

D.  Pb²⁺ ions lose electrons at the cathode (negative electrode).