When 5.175 g of lead are heated at 300°C, the lead reacts with the oxygen in the air to produce 5.708 g of an oxide of lead. This is the only product.
What is the equation for this reaction?
Answer (3)
Mass of oxygen used is 5.708 – 5.175 g = 0.533 g Moles of lead reacting = (5.175/207) mol = 0.025 mol Moles of oxygen reacting = (0.533/32) mol = 0.0167 mol ∴0.025 mol of Pb react with 0.0167 mol of O2to give product ∴1.5 mol of Pb react with 1 mol of O2to give product ∴3 mol of Pb react with 2 mol of O2to give product 3Pb+ 2O2→Pb3O4You do not have the information to write the full equation but as you know there is only one product and this has 3 lead atoms and 4 oxygen you can suggest a formula. ;
The reaction between lead and oxygen produces lead oxide (PbO) as the only product. 2Pb + O₂ → 2PbO
To write the balanced chemical equation for the reaction between lead and oxygen, we can follow these steps:
Step 1: Write the given information:
Mass of lead (Pb) = 5.175 g
Mass of lead oxide (PbO) produced = 5.708 g
Step 2: Calculate the change in mass (mass of product - mass of reactant):
Change in mass = Mass of product - Mass of reactant
Change in mass = 5.708 g - 5.175 g
Change in mass = 0.533 g
Step 3: Determine the stoichiometry:
The balanced chemical equation will have the following form:
aPb + bO₂ → cPbO
Step 4: Convert masses to moles:
To find the stoichiometric coefficients (a, b, and c), we need to convert the masses of lead and lead oxide to moles.
Molar mass of Pb (lead) = 207.2 g/mol
Molar mass of PbO (lead oxide) = 223.2 g/mol (Pb: 207.2 g/mol + O: 16.0 g/mol)
Moles of Pb = Mass of Pb / Molar mass of Pb
Moles of Pb = 5.175 g / 207.2 g/mol ≈ 0.02498 moles
Moles of PbO = Mass of PbO / Molar mass of PbO
Moles of PbO = 5.708 g / 223.2 g/mol ≈ 0.02556 moles
Step 5: Determine the stoichiometric coefficients:
The stoichiometric coefficients can be determined by dividing the moles of each substance by the smallest number of moles (to get the simplest whole-number ratio ).
a (Pb) = Moles of Pb / Smallest number of moles ≈ 0.02498 moles / 0.02498 moles ≈ 1
b (O₂) = Moles of PbO / Smallest number of moles ≈ 0.02556 moles / 0.02498 moles ≈ 1
c (PbO) = Moles of PbO / Smallest number of moles ≈ 0.02556 moles / 0.02498 moles ≈ 1
Step 6: Write the balanced chemical equation:
The balanced chemical equation for the reaction is:
2Pb + O₂ → 2PbO
The reaction between lead and oxygen produces** lead oxide** (PbO) as the only product.
Learn more about** lead oxide **from the link given below.
https://brainly.com/question/6529765
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The balanced chemical equation for the reaction between lead and oxygen is 2Pb + O₂ → 2PbO. This shows that two moles of lead react with one mole of oxygen to produce two moles of lead(II) oxide. The reaction confirms the conservation of mass, as indicated by balancing the number of atoms of each element on both sides of the equation.
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