9. The balanced equation below represents a double replacement reaction. PbCl_(2)(aq)+Na_(2)CrO_(4)(aq)arrow PbCrO_(3)(s)+2NaCl(aq) What is the total number of moles of NaCl formed when 2 moles of Na_(2)CrO_(4) reacts completely? 1 mole 2 moles 3 moles 4 moles

The balanced chemical equation given is:<br />\[ PbCl_{2}(aq) + Na_{2}CrO_{4}(aq) \rightarrow PbCrO_{3}(s) + 2NaCl(aq) \]<br />From the equation, we can see that 1 mole of \( PbCl_{2} \) reacts with 1 mole of \( Na_{2}CrO_{4} \) to produce 2 moles of \( NaCl \). Therefore, if 2 moles of \( Na_{2}CrO_{4} \) react completely, 4 moles of \( NaCl \) will be formed. Hence, the correct answer is 4 moles.