how to calculate ? when 21g of magnesium carbonate was heated , magnesium oxide produced . carbon dioxide also released. what is the volume of carbon dioxide released ?
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Given that 21kg of magnesium carbonate is heated, calculate the mass of magnesium oxide formed.
7,5g
I need the answer
To calculate the volume of carbon dioxide released, we need to know the mass of magnesium carbonate, its molar mass, and the balanced chemical equation for its decomposition.
Here's the step-by-step process:
1. Identify the molar mass of magnesium carbonate (MgCO3).
- Magnesium (Mg) has a molar mass of 24.31 g/mol.
- Carbon (C) has a molar mass of 12.01 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol.
- Therefore, the molar mass of MgCO3 is: (24.31 + 12.01 + (16.00 x 3)) g/mol = 84.31 g/mol.
2. Determine the number of moles of magnesium carbonate.
- Mass (m) = 21 g.
- Number of moles (n) is calculated using the formula: n = m / Molar mass.
- Therefore, n = 21 g / 84.31 g/mol = 0.2491 mol.
3. Examine the balanced chemical equation for the decomposition of magnesium carbonate.
The balanced equation is: MgCO3(s) -> MgO(s) + CO2(g)
4. Determine the stoichiometric ratio between magnesium carbonate and carbon dioxide.
- From the balanced equation, we see that for every 1 mol of MgCO3, 1 mol of CO2 is produced.
5. Calculate the number of moles of carbon dioxide produced.
- Since the stoichiometric ratio is 1:1, the number of moles of carbon dioxide (CO2) released will be the same as the number of moles of magnesium carbonate (MgCO3).
- The number of moles of CO2 released = 0.2491 mol.
6. Determine the volume of carbon dioxide using the ideal gas law.
- The ideal gas law equation is: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L.atm/mol.K), and T is the temperature in Kelvin.
- Assuming constant temperature and pressure, we can rearrange the equation to solve for volume: V = (nRT) / P.
- Assuming standard temperature and pressure (STP), P = 1 atm.
- Assuming room temperature (around 298 K), we can use these values in the equation: V = (0.2491 mol x 0.0821 L.atm/mol.K x 298 K) / 1 atm.
7. Calculate the actual volume of carbon dioxide.
- V = 0.2491 mol x 0.0821 L.atm/mol.K x 298 K = 6.166 L (rounded to three decimal places).
Therefore, the volume of carbon dioxide released when 21 g of magnesium carbonate decomposes is approximately 6.166 liters.