Question

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Explanation:

Step1: Analyze the balanced equation

The balanced chemical equation is \(2K + Cl_2
ightarrow 2KCl\). From the equation, the mole ratio of \(Cl_2\) to \(KCl\) is \(1:2\) (1 mole of \(Cl_2\) produces 2 moles of \(KCl\)).

Step2: Check each step

• Step 1: It's just writing the given mass of \(Cl_2\), which is a starting point, no error here.
• Step 2: Converting grams of \(Cl_2\) to moles using molar mass (\(70.915\ g/mol\) for \(Cl_2\)) is correct. The conversion factor \(\frac{1\ mole\ Cl_2}{70.915\ g\ Cl_2}\) is appropriate.
• Step 3: The mole ratio from the balanced equation is \(1\ mole\ Cl_2 : 2\ moles\ KCl\). But the student has the ratio as \(\frac{1\ mole\ KCl}{2\ moles\ Cl_2}\), which is inverted. It should be \(\frac{2\ moles\ KCl}{1\ mole\ Cl_2}\) to correctly convert moles of \(Cl_2\) to moles of \(KCl\).

Answer:

Step 3 is incorrect because the mole ratio used is inverted. The correct mole ratio from the balanced equation \(2K + Cl_2
ightarrow 2KCl\) is \(\frac{2\ moles\ KCl}{1\ mole\ Cl_2}\), but the student used \(\frac{1\ mole\ KCl}{2\ moles\ Cl_2}\).