Question

# When potassium dichromate is heated, one of the products are :A.${{K}_{2}}O$B.$C{{r}_{2}}{{O}_{5}}$C.${{O}_{3}}$D.${{O}_{2}}$

Hint: ${{K}_{2}}C{{r}_{2}}{{O}_{7}}$ is an orange red crystalline solid and it decomposes on strong heating and a yellow coloured compound is obtained along with an oxide of chromium and a gas which is essential for combustion. Now, by using this you can easily answer the given question.

-It is known to you that when potassium dichromate (${{K}_{2}}C{{r}_{2}}{{O}_{7}}$) is heated strongly it gets decomposed into a yellow coloured compound, an oxide of chromium which is green in colour and oxygen gas.
-The yellow coloured compound is potassium chromate (${{K}_{2}}Cr{{O}_{4}}$) and the oxide of chromium is chromic oxide ($C{{r}_{2}}{{O}_{3}}$). The reaction is as follows:
$4{{K}_{2}}C{{r}_{2}}{{O}_{7}}\xrightarrow{\Delta }4{{K}_{2}}Cr{{O}_{4}}+2C{{r}_{2}}{{O}_{3}}+3{{O}_{2}}$.

Hence option D is correct.

-When potassium dichromate is heated with conc. Sulphuric acid and a soluble metal chloride, orange red vapors of chromyl chloride are evolved. When these vapors are passed through sodium hydroxide solution, yellow coloration is obtained. This reaction is used in the detection of $C{{l}^{-}}$ ions in qualitative analysis and the test is known as chromyl chloride test.