Question
Calcium carbonate (CaCO3
) can undergo a chemical reaction to produce calcium oxide (CaO
) and carbon dioxide (CO2
). Which possible masses of calcium oxide and carbon dioxide can form when 200g of calcium carbonate undergoes this chemical reaction?(1 point)
Responses
40g CaO
and 12g CO2
40g cap c A cap o and 12g cap c cap o sub 2
56g CaO
and 44g CO2
56g cap c A cap o and 44g cap c cap o sub 2
200g CaO
and 200g CO2
200g cap c A cap o and 200g cap c cap o sub 2
112g CaO
and 88g CO2
) can undergo a chemical reaction to produce calcium oxide (CaO
) and carbon dioxide (CO2
). Which possible masses of calcium oxide and carbon dioxide can form when 200g of calcium carbonate undergoes this chemical reaction?(1 point)
Responses
40g CaO
and 12g CO2
40g cap c A cap o and 12g cap c cap o sub 2
56g CaO
and 44g CO2
56g cap c A cap o and 44g cap c cap o sub 2
200g CaO
and 200g CO2
200g cap c A cap o and 200g cap c cap o sub 2
112g CaO
and 88g CO2
Answers
GPT-4o mini
To determine the possible masses of calcium oxide (CaO) and carbon dioxide (CO₂) produced from the decomposition of calcium carbonate (CaCO₃), we can follow the stoichiometry of the reaction.
The balanced chemical equation for the decomposition of calcium carbonate is:
\[ \text{CaCO}_3 (s) \rightarrow \text{CaO} (s) + \text{CO}_2 (g) \]
From this equation, we can see that 1 mole of calcium carbonate produces 1 mole of calcium oxide and 1 mole of carbon dioxide.
1. **Calculate the molar masses:**
- Molar mass of CaCO₃ = 40.08 (Ca) + 12.01 (C) + 3 × 16.00 (O) = 100.09 g/mol
- Molar mass of CaO = 40.08 (Ca) + 16.00 (O) = 56.08 g/mol
- Molar mass of CO₂ = 12.01 (C) + 2 × 16.00 (O) = 44.01 g/mol
2. **Determine the number of moles of CaCO₃ in 200 g:**
\[
\text{Moles of CaCO}_3 = \frac{200 \, \text{g}}{100.09 \, \text{g/mol}} \approx 1.996 \, \text{moles}
\]
3. **Using the reaction ratio:**
From the balanced equation, 1 mole of CaCO₃ produces 1 mole of CaO and 1 mole of CO₂.
- Moles of CaO produced = moles of CaCO₃ = 1.996 moles
- Moles of CO₂ produced = moles of CaCO₃ = 1.996 moles
4. **Calculate the masses of CaO and CO₂ produced:**
- Mass of CaO:
\[
\text{Mass of CaO} = 1.996 \, \text{moles} \times 56.08 \, \text{g/mol} \approx 112 \, \text{g}
\]
- Mass of CO₂:
\[
\text{Mass of CO}_2 = 1.996 \, \text{moles} \times 44.01 \, \text{g/mol} \approx 88 \, \text{g}
\]
Based on this analysis, the masses produced when 200g of calcium carbonate decomposes are approximately:
\[ 112 \, \text{g CaO} \text{ and } 88 \, \text{g CO}_2 \]
Thus, the correct response is:
**112g CaO and 88g CO₂**.
The balanced chemical equation for the decomposition of calcium carbonate is:
\[ \text{CaCO}_3 (s) \rightarrow \text{CaO} (s) + \text{CO}_2 (g) \]
From this equation, we can see that 1 mole of calcium carbonate produces 1 mole of calcium oxide and 1 mole of carbon dioxide.
1. **Calculate the molar masses:**
- Molar mass of CaCO₃ = 40.08 (Ca) + 12.01 (C) + 3 × 16.00 (O) = 100.09 g/mol
- Molar mass of CaO = 40.08 (Ca) + 16.00 (O) = 56.08 g/mol
- Molar mass of CO₂ = 12.01 (C) + 2 × 16.00 (O) = 44.01 g/mol
2. **Determine the number of moles of CaCO₃ in 200 g:**
\[
\text{Moles of CaCO}_3 = \frac{200 \, \text{g}}{100.09 \, \text{g/mol}} \approx 1.996 \, \text{moles}
\]
3. **Using the reaction ratio:**
From the balanced equation, 1 mole of CaCO₃ produces 1 mole of CaO and 1 mole of CO₂.
- Moles of CaO produced = moles of CaCO₃ = 1.996 moles
- Moles of CO₂ produced = moles of CaCO₃ = 1.996 moles
4. **Calculate the masses of CaO and CO₂ produced:**
- Mass of CaO:
\[
\text{Mass of CaO} = 1.996 \, \text{moles} \times 56.08 \, \text{g/mol} \approx 112 \, \text{g}
\]
- Mass of CO₂:
\[
\text{Mass of CO}_2 = 1.996 \, \text{moles} \times 44.01 \, \text{g/mol} \approx 88 \, \text{g}
\]
Based on this analysis, the masses produced when 200g of calcium carbonate decomposes are approximately:
\[ 112 \, \text{g CaO} \text{ and } 88 \, \text{g CO}_2 \]
Thus, the correct response is:
**112g CaO and 88g CO₂**.