When 0.100 mole of BaCl_2 reacts completely with excess Na_2SO_4 according to the equation BaCl_2 + Na_2SO_4 → BaSO_4 + 2NaCl, how many moles of BaSO_4 are produced?

• A. 0.200 mole
• B. 0.0250 mole
• C. 0.0500 mole
• D. 0.100 mole

Answer: (D)

Verified step by step guidance

1. Write down the balanced chemical equation: \(\text{BaCl}_2 + \text{Na}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{NaCl}\).
2. Identify the mole ratio between BaCl\(_2\) and BaSO\(_4\) from the balanced equation. Here, 1 mole of BaCl\(_2\) produces 1 mole of BaSO\(_4\).
3. Note the amount of BaCl\(_2\) given: 0.100 mole.
4. Since the reaction goes to completion and Na\(_2\)SO\(_4\) is in excess, all BaCl\(_2\) will react, producing an equivalent amount of BaSO\(_4\) based on the mole ratio.
5. Therefore, the moles of BaSO\(_4\) produced will be equal to the moles of BaCl\(_2\) reacted, which is 0.100 mole.