
What happens when ${\text{S}}{{\text{O}}_2}$ is passed through acidified ${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$ solution?
Answer
432k+ views
Hint- Here, we will proceed by giving some details about sulfur dioxide and potassium dichromate. Then, we will be writing down the balanced chemical reaction involved in which potassium dichromate behaves as a strong oxidising agent.
Complete answer:
Sulfur dioxide is a poisonous gas and is responsible for the scent of matches burned. It is naturally emitted by volcanic activity and is created as a by-product of copper extraction and the burning of sulfur-contaminated fossil fuels. In appearance, this gas is colourless.
Potassium dichromate solution (${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$) is an inorganic, orange to red coloured compound that releases poisonous fumes of chromium when heated. Potassium dichromate is highly corrosive, and is a strong oxidizer. This material is used in wood preservatives, in pigment manufacturing and in photomechanical processes, but is substituted primarily by sodium dichromate.
When sulfur dioxide (${\text{S}}{{\text{O}}_2}$) is passed through acidified (in the presence of sulphuric acid i.e., ${{\text{H}}_2}{\text{S}}{{\text{O}}_4}$) potassium dichromate solution (${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$), potassium sulfate (${{\text{K}}_2}{\text{S}}{{\text{O}}_4}$) and chromium sulphate (${\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3}$) are formed along with water molecules. The balanced chemical reaction of this process is shown below.
${\text{3S}}{{\text{O}}_2} + {{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7} + {{\text{H}}_2}{\text{S}}{{\text{O}}_4} \to {{\text{K}}_2}{\text{S}}{{\text{O}}_4} + {\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3} + {{\text{H}}_2}{\text{O}}$
Potassium dichromate (${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$) is a strong oxidising agent and hence the sulfur dioxide (${\text{S}}{{\text{O}}_2}$) gets oxidised to sulfate (${\text{S}}{{\text{O}}_4}^{2 - }$), the ${\text{C}}{{\text{r}}^{ + 6}}$ in potassium dichromate (orange coloured) gets reduced to ${\text{C}}{{\text{r}}^{ + 3}}$ in chromium sulphate (${\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3}$) which is green coloured compound.
Potassium sulfate is a potassium source that is moderately water and acid soluble for use consistent with sulfates. Sulfate compounds are sulfuric acid salts or esters formed by substituting one or both of the hydrogens with the metal. In uses such as water treatment, most metal sulfate compounds are readily soluble in water, unlike the fluorides and oxides that appear to be insoluble. Organometallic forms are soluble in organic solutions, and in aqueous and organic solutions at times.
Chromium sulfate typically refers to inorganic compounds that are known commercially as chromium sulfate base.
Note- Chromium sulfate is used in paints, inks, ceramics and garment dyeing processes. They are non-combustible. In this particular problem, the oxidation number of chromium in ${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$ is given by $2\left( { + 1} \right) + 2x + 7\left( { - 2} \right) = 0 \Rightarrow 2x = 14 - 2 \Rightarrow x = 6$ and in ${\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3}$ is given by $2y + 3\left( { - 2} \right) = 0 \Rightarrow 2y = 6 \Rightarrow y = 3$.
Complete answer:
Sulfur dioxide is a poisonous gas and is responsible for the scent of matches burned. It is naturally emitted by volcanic activity and is created as a by-product of copper extraction and the burning of sulfur-contaminated fossil fuels. In appearance, this gas is colourless.
Potassium dichromate solution (${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$) is an inorganic, orange to red coloured compound that releases poisonous fumes of chromium when heated. Potassium dichromate is highly corrosive, and is a strong oxidizer. This material is used in wood preservatives, in pigment manufacturing and in photomechanical processes, but is substituted primarily by sodium dichromate.
When sulfur dioxide (${\text{S}}{{\text{O}}_2}$) is passed through acidified (in the presence of sulphuric acid i.e., ${{\text{H}}_2}{\text{S}}{{\text{O}}_4}$) potassium dichromate solution (${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$), potassium sulfate (${{\text{K}}_2}{\text{S}}{{\text{O}}_4}$) and chromium sulphate (${\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3}$) are formed along with water molecules. The balanced chemical reaction of this process is shown below.
${\text{3S}}{{\text{O}}_2} + {{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7} + {{\text{H}}_2}{\text{S}}{{\text{O}}_4} \to {{\text{K}}_2}{\text{S}}{{\text{O}}_4} + {\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3} + {{\text{H}}_2}{\text{O}}$
Potassium dichromate (${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$) is a strong oxidising agent and hence the sulfur dioxide (${\text{S}}{{\text{O}}_2}$) gets oxidised to sulfate (${\text{S}}{{\text{O}}_4}^{2 - }$), the ${\text{C}}{{\text{r}}^{ + 6}}$ in potassium dichromate (orange coloured) gets reduced to ${\text{C}}{{\text{r}}^{ + 3}}$ in chromium sulphate (${\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3}$) which is green coloured compound.
Potassium sulfate is a potassium source that is moderately water and acid soluble for use consistent with sulfates. Sulfate compounds are sulfuric acid salts or esters formed by substituting one or both of the hydrogens with the metal. In uses such as water treatment, most metal sulfate compounds are readily soluble in water, unlike the fluorides and oxides that appear to be insoluble. Organometallic forms are soluble in organic solutions, and in aqueous and organic solutions at times.
Chromium sulfate typically refers to inorganic compounds that are known commercially as chromium sulfate base.
Note- Chromium sulfate is used in paints, inks, ceramics and garment dyeing processes. They are non-combustible. In this particular problem, the oxidation number of chromium in ${{\text{K}}_2}{\text{C}}{{\text{r}}_2}{{\text{O}}_7}$ is given by $2\left( { + 1} \right) + 2x + 7\left( { - 2} \right) = 0 \Rightarrow 2x = 14 - 2 \Rightarrow x = 6$ and in ${\text{C}}{{\text{r}}_2}{\left( {{\text{S}}{{\text{O}}_4}} \right)_3}$ is given by $2y + 3\left( { - 2} \right) = 0 \Rightarrow 2y = 6 \Rightarrow y = 3$.
Recently Updated Pages
The correct geometry and hybridization for XeF4 are class 11 chemistry CBSE

Water softening by Clarks process uses ACalcium bicarbonate class 11 chemistry CBSE

With reference to graphite and diamond which of the class 11 chemistry CBSE

A certain household has consumed 250 units of energy class 11 physics CBSE

The lightest metal known is A beryllium B lithium C class 11 chemistry CBSE

What is the formula mass of the iodine molecule class 11 chemistry CBSE

Trending doubts
Is Cellular respiration an Oxidation or Reduction class 11 chemistry CBSE

In electron dot structure the valence shell electrons class 11 chemistry CBSE

What is the Pitti Island famous for ABird Sanctuary class 11 social science CBSE

State the laws of reflection of light

One Metric ton is equal to kg A 10000 B 1000 C 100 class 11 physics CBSE

Difference Between Prokaryotic Cells and Eukaryotic Cells
