Calculate the weight of lime (CaO) obtained by heating 225kg of 95% pure lime stone (`CaCO_3`).
`CaCO_3​→CaO+CO_2` ​

Explanation

To calculate the weight of lime (CaO) obtained by heating 225 kg of 95% pure limestone (CaCO3), we can follow these steps:

### Step 1: Calculate the weight of pure CaCO3 in the limestone
First, we need to determine the amount of pure CaCO3 in the 225 kg of limestone. Since the limestone is 95% pure, we can calculate the weight of pure CaCO3 as follows:

\[ \text{Weight of pure } CaCO_3 = \frac{95}{100} \times 225 \text{ kg} \]

Calculating this gives:

\[ \text{Weight of pure } CaCO_3 = 0.95 \times 225 = 213.75 \text{ kg} \]

### Step 2: Write the decomposition reaction
The decomposition of calcium carbonate (CaCO3) can be represented by the following chemical equation:

\[ CaCO_3 \rightarrow CaO + CO_2 \]

From this equation, we can see that 1 mole of CaCO3 produces 1 mole of CaO.

### Step 3: Calculate the molar masses
Next, we need the molar masses of CaCO3 and CaO:
- Molar mass of CaCO3 = 100 g/mol
- Molar mass of CaO = 56 g/mol

### Step 4: Set up the conversion ratio
From the molar masses, we can establish the conversion ratio:

\[ 100 \text{ g of } CaCO_3 \text{ produces } 56 \text{ g of } CaO \]

### Step 5: Calculate the weight of CaO produced
Now we can calculate the amount of CaO produced from the pure CaCO3 we found in step 1. We will use the conversion ratio to find the weight of CaO produced from 213.75 kg of CaCO3:

\[ \text{Weight of } CaO = \left( \frac{56}{100} \right) \times 213.75 \text{ kg} \]

Calculating this gives:

\[ \text{Weight of } CaO = 0.56 \times 213.75 = 119.7 \text{ kg} \]

### Final Answer
The weight of lime (CaO) obtained by heating 225 kg of 95% pure limestone is **119.7 kg**.

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