Which of the following would be the correct set up to determine the number of formula units in 3.26g of MgCl_(2) 3.26gMgCl_(2)times (1molMgCl_(2))/(95.2gMgCl_(2))times (1molMgCl_(2))/(6.02times 10^23)fom unts 3.26gMgCl_(2)times (95.2gMgCl_(2))/(1molMgCl_(2))times (1molMgCl_(2))/(6.02times 10^23)fom units 3.26gMgCl_(2)times (1molMgCl_(2))/(95.2gMgCl_(2))times (6.02times 10^23tomunts)/(1molMgCl_(2)) 95.2gMgCl_(2)times (1molMgCl_(2))/(3.26gMgCl_(2))times (6.02times 10^23fomunts)/(1molMgCl_(2))

To determine the number of formula units in 3.26g of \( MgCl_2 \), you need to follow these steps:<br /><br />1. Convert grams of \( MgCl_2 \) to moles using the molar mass of \( MgCl_2 \).<br />2. Convert moles of \( MgCl_2 \) to formula units using Avogadro's number.<br /><br />The correct setup for this calculation is:<br /><br />\[ 3.26 \, \text{g} \, MgCl_2 \times \frac{1 \, \text{mol} \, MgCl_2}{95.2 \, \text{g} \, MgCl_2} \times \frac{6.02 \times 10^{23} \, \text{formula units}}{1 \, \text{mol} \, MgCl_2} \]<br /><br />So, the correct option is:<br /><br />\[ 3.26gMgCl_{2}\times \frac {1molMgCl_{2}}{95.2gMgCl_{2}}\times \frac {6.02\times 10^{23} \, \text{formula units}}{1molMgCl_{2}} \]