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Sulphate salt metal oxide and SO(3)(or S...

Sulphate salt metal oxide and `SO_(3)(or SO_(2)+(1)/(2)O_(2))` on heating:

A

`K_(2)SO_(4)`

B

`CaSO_(4)`

C

`MgSO_(4)`

D

`(NH_(4))_(2)SO_(4)`

Text Solution

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The correct Answer is:
To solve the question regarding the thermal decomposition of sulphate salts, we will analyze the given compounds and their behavior upon heating. The question states that sulphate salts of metal oxides decompose to form SO3 or SO2 along with half O2. ### Step-by-Step Solution: 1. **Identify the Compounds**: The compounds given are K2SO4 (Potassium Sulfate), CaSO4 (Calcium Sulfate), MgSO4 (Magnesium Sulfate), and NH4SO4 (Ammonium Sulfate). 2. **Evaluate Thermal Stability**: - **K2SO4** and **NH4SO4**: These are alkali metal and ammonium sulphates, respectively. Both of these compounds are known to be thermally stable and do not decompose upon heating. Therefore, they cannot be the answer. - **CaSO4** and **MgSO4**: These are alkaline earth metal sulphates. They are known to decompose upon heating. 3. **Heating of CaSO4 and MgSO4**: - When heated, both calcium sulfate (CaSO4) and magnesium sulfate (MgSO4) decompose to form their respective metal oxides (CaO and MgO) and release SO3 gas. - The reactions can be represented as: - For CaSO4: \[ \text{CaSO}_4 \xrightarrow{\text{heat}} \text{CaO} + \text{SO}_3 \] - For MgSO4: \[ \text{MgSO}_4 \xrightarrow{\text{heat}} \text{MgO} + \text{SO}_3 \] 4. **Conclusion**: Since K2SO4 and NH4SO4 do not decompose upon heating, the only viable options are CaSO4 and MgSO4, which do decompose to form metal oxides and SO3. Thus, the correct answer is **CaSO4 and MgSO4**.
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