Question

Balance the following equation:

K2CrO4+Na2SO3+HCl?KCl+Na2SO4+CrCl3+H2O

Generally coefficients of 1 are omitted from balanced chemical equations. When entering your answer, include coefficients of 1 as required for grading purposes.

Enter the coefficients for each compound, separated by commas, in the order in which they appear in the equation (e.g., 1,2,3,4,5,6,7).

Part B

In the process of oxidizing I? to I2, SO42? is reduced to SO2. How many moles of SO2 are produced in the formation of one mole of I2?

Express your answer numerically in moles.

Answer 1

Answer: a) $2K_2CrO_4+3Na_2SO_3+10HCl\rightarrow 4KCl+3Na_2SO_4+2CrCl_3+5H_2O$

b) 1 mole of $SO_2$ is produced.

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

The skeletal equation is:

$K_2CrO_4+Na_2SO_3+HCl\rightarrow KCl+Na_2SO_4+CrCl_3 +H_2O$

The balanced equation will be:

$2K_2CrO_4+3Na_2SO_3+10HCl\rightarrow 4KCl+3Na_2SO_4+2CrCl_3+5H_2O$

Thus the coefficients are 2, 3 , 10 , 4 , 3 , 2 and 5.

b) Oxidation: $2I-^-\rightarrow I_2+2e-^-$

Reduction: $SO_4^{2-}+2e^-+4H^+\rightarrow SO_2+2H_2O

$

Net reaction:  $2I-^-+SO_4^{2-}+4H^+\rightarrow I_2+SO_2+2H_2O$

When 1 mole of $I_2$ is produced, 1 mole of $SO_2$ is produced.

Answer 2

The balanced equation of the given reaction is as follows:

• 2 K₂CrO₄ + 3 Na₂SO₃ + 10 HCl ----> 4 KCl + 3 Na₂SO₄ + 2 CrCl₃ + 5 H₂O

When one mole of I₂ is formed, one mole of SO₂ is produced.

How to balance a chemical equation

In balancing a chemical equation, numerical coefficients are added in front of the reactants and/or products to ensure that the moles of atoms of elements reacting are equal to moles of atoms of elements produced.

How can the equation of the given reaction be balanced?

The balanced equation of the given reaction is as follows:

2 K₂CrO₄ + 3 Na₂SO₃ + 10 HCl ----> 4 KCl + 3 Na₂SO₄ + 2 CrCl₃ + 5 H₂O

Thus, the numerical coefficients are: 2, 3, 10, 4, 3, 2, 5

How is the moles of SO₂ produce determined when I⁻ is oxidized to I₂?

The balanced net ionic equation of the reaction is given below:

2 I⁻ (aq) + SO₄²⁻ (aq) + 4 H⁺ ---> I₂ (s) + SO₂ (g) + 2 H₂O

From the equation of the reaction, in the formation of one mole of I₂, one mole of SO₂ is produced.

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