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An aluminium atom has the atomic number 13 and the mass number 27 - Edexcel - GCSE Chemistry Combined Science - Question 6 - 2019 - Paper 1

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An aluminium atom has the atomic number 13 and the mass number 27. Which row shows the numbers of subatomic particles present in an aluminium ion, Al$^{3+}$? | prot... show full transcript

Worked Solution & Example Answer:An aluminium atom has the atomic number 13 and the mass number 27 - Edexcel - GCSE Chemistry Combined Science - Question 6 - 2019 - Paper 1

Step 1

Which row shows the numbers of subatomic particles present in an aluminium ion, Al$^{3+}$?

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Answer

To find the number of subatomic particles in the aluminium ion, we consider the atomic number and mass number:

  • The atomic number of aluminium is 13, which means it has 13 protons.
  • The mass number is 27, which indicates the total number of protons and neutrons. Therefore, the number of neutrons is calculated as: neutrons=mass number−atomic number=27−13=14\text{neutrons} = \text{mass number} - \text{atomic number} = 27 - 13 = 14
  • The aluminium ion is Al3+^{3+}, indicating it has lost 3 electrons; thus, the number of electrons is: electrons=13−3=10\text{electrons} = 13 - 3 = 10 In summary, the aluminium ion has:
  • Protons: 13
  • Neutrons: 14
  • Electrons: 10 The correct row is B (13, 14, 10).

Step 2

Starting with 1.35g of magnesium, calculate the maximum mass of magnesium oxide that could be formed in this reaction.

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Answer

To calculate the maximum mass of magnesium oxide (MgO) that can be formed from 1.35g of magnesium, we follow these steps:

  1. Calculate the number of moles of magnesium: The molar mass of Mg is 24.0 g/mol. moles of Mg=massmolar mass=1.35 g24.0 g/mol≈0.0563 mol\text{moles of Mg} = \frac{\text{mass}}{\text{molar mass}} = \frac{1.35 \, \text{g}}{24.0 \, \text{g/mol}} \approx 0.0563 \, \text{mol}

  2. Determine the moles of magnesium oxide produced: According to the balanced equation: 2Mg+O2→2MgO2Mg + O_2 \rightarrow 2MgO From the equation, 2 moles of Mg produce 2 moles of MgO, hence: moles of MgO=0.0563 mol\text{moles of MgO} = 0.0563 \, \text{mol}

  3. Calculate the mass of magnesium oxide produced: The molar mass of MgO is: molar mass of MgO=24.0 g/mol+16.0 g/mol=40.0 g/mol\text{molar mass of MgO} = 24.0 \, \text{g/mol} + 16.0 \, \text{g/mol} = 40.0 \, \text{g/mol} Therefore, the mass of MgO produced is: mass of MgO=moles×molar mass=0.0563 mol×40.0 g/mol≈2.25 g\text{mass of MgO} = \text{moles} \times \text{molar mass} = 0.0563 \, \text{mol} \times 40.0 \, \text{g/mol} \approx 2.25 \, \text{g} Thus, the maximum mass of magnesium oxide that could be formed is approximately 2.25g.

Step 3

Write the balanced equation for this reaction.

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Answer

The balanced equation for the reaction between chlorine and hydrogen to form hydrogen chloride is: Cl2+H2→2HClCl_2 + H_2 \rightarrow 2HCl This equation reflects the law of conservation of mass, ensuring that the number of atoms for each element is the same on both sides of the equation.

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