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MAXImum [283]
2 years ago
8

MgCl2 (aq) + K2SO4 (aq) --> 2KCl (aq) + MgSO4 (s)

Chemistry
1 answer:
vova2212 [387]2 years ago
4 0

Answer:

\boxed {\boxed {\sf 9.6 \ mol \ KCl}}

Explanation:

We must use stoichiometry to solve this, which is the calculation of reactants and products in a reaction using ratios.

Let's analyze the reaction given.

MgCl_2 _{(aq)} + K_2SO_4 _{(aq)}  \rightarrow 2KCl _{(aq)} + MgSO_4 _{(s)}

Now, look at the coefficients, or numbers in front of the molecule formulas. If there isn't a coefficient, then a 1 is implied.

We want to find how many moles of potassium chloride (KCl) are produced from 4.8 moles of magnesium chloride (MgCl₂). Check the coefficients for these molecules.

  • MgCl₂: no coefficient= coefficient of 1
  • KCl: coefficient of 2

The coefficient represents the number of moles. Therefore, 1 mole of magnesium chloride produces 2 moles of potassium chloride. We can set up a ratio using this information.

\frac { 1 \ mol \ MgCl_2} {2 \ mol \ KCl}

Multiply by the given number of moles of magnesium chloride: 4.8

4.8 \ mol \ MgCl_2 *\frac { 1 \ mol \ MgCl_2} {2 \ mol \ KCl}

Flip the ratio so the moles of magnesium chloride cancel out.

4.8 \ mol \ MgCl_2 *\frac {2 \ mol \ KCl} { 1 \ mol \ MgCl_2}

4.8  *\frac {2 \ mol \ KCl} { 1 \ } }

4.8   * {2 \ mol \ KCl}

9.6 \ mol \ KCl

<u>9.6 moles of potassium chloride are produced </u>from 4.8 moles of magnesium chloride.

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