100 g of a pure sample of `CaCO_3` is treated a with `500 cm^(3)` of `M/2` HCI solution. Calculate the of `CO_2` that will be evolved at S.T.P.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between calcium carbonate (CaCO₃) and hydrochloric acid (HCl) can be represented as:
\[ \text{CaCO}_3 + 2 \text{HCl} \rightarrow \text{CaCl}_2 + \text{H}_2\text{O} + \text{CO}_2 \]

### Step 2: Calculate the number of moles of CaCO₃
Given that we have 100 grams of calcium carbonate (CaCO₃), we need to find the number of moles. The molar mass of CaCO₃ is approximately 100 g/mol.
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