Question

write the balanced chemical reaction for the dehydration of magnesium sulfate heptahydrate. include physical states.

balanced chemical reaction:

determine the theoretical mass of magnesium sulfate and the theoretical mass of water vapor that should be produced from the complete dehydration of 8.207 g of magnesium sulfate heptahydrate. the molar mass of magnesium sulfate heptahydrate is 246.472 g/mol, the molar mass of magnesium sulfate is 120.367 g/mol, and the molar mass of water is 18.015 g/mol. use the reaction stoichiometry to calculate the masses of the anhydrous compound and water vapor.

mass of magnesium sulfate:

mass of water vapor:

Explanation:

Write the balanced chemical equation

Using the Dehydration Reaction and Anhydrous Salts knowledge points

$$ \text{MgSO}_4\cdot7\text{H}_2\text{O(s)} ightarrow \text{MgSO}_4\text{(s)} + 7\text{H}_2\text{O(g)} $$

Calculate moles of magnesium sulfate heptahydrate

Using the Stoichiometry knowledge point

$$ n_{\text{hydrate}} = \frac{8.207\text{ g}}{246.472\text{ g/mol}} \approx 0.0332979\text{ mol} $$

Calculate the theoretical mass of anhydrous magnesium sulfate

Using the Stoichiometry knowledge point

$$
LATEXBLOCK0
$$

Calculate the theoretical mass of water vapor

Using the Stoichiometry knowledge point

$$
LATEXBLOCK1
$$

Answer:

Question 1

balanced chemical reaction: \(\text{MgSO}_4\cdot7\text{H}_2\text{O(s)}
ightarrow \text{MgSO}_4\text{(s)} + 7\text{H}_2\text{O(g)}\)

Question 2

mass of magnesium sulfate: \(4.008\text{ g}\)

Question 3

mass of water vapor: \(4.199\text{ g}\)