Pb(NO_(3))_(2)(aq)+2KI(aq)arrow PbI_(2)(s)+2KNO_(3) (aq) How many liters of KNO_(3) are produced if 2.65 L of Pb(NO_(3))_(2) are used? 4.29L of KNO_(3) 3.29L of KNO_(3) 6.29L of KNO_(3) 5.29L of KNO_(3)

To solve this problem, we need to use the concept of stoichiometry and the balanced chemical equation.<br /><br />Given information:<br />- The balanced chemical equation is: $Pb(NO_{3})_{2}(aq)+2KI(aq)\rightarrow PbI_{2}(s)+2KNO_{3}(aq)$<br />- 2.65 L of $Pb(NO_{3})_{2}$ are used.<br /><br />Step 1: Determine the molar ratio between $Pb(NO_{3})_{2}$ and $KNO_{3}$.<br />From the balanced equation, we can see that 1 mole of $Pb(NO_{3})_{2}$ produces 2 moles of $KNO_{3}$.<br /><br />Step 2: Calculate the volume of $KNO_{3}$ produced.<br />Since the molar ratio is 1:2, the volume of $KNO_{3}$ produced will be twice the volume of $Pb(NO_{3})_{2}$ used.<br /><br />Volume of $KNO_{3}$ produced = 2 × 2.65 L = 5.29 L<br /><br />Therefore, the correct answer is 5.29 L of $KNO_{3}$.