a popular sports drink has 30.43 g of the sugar sucrose in 500. ml of the beverage. the formula for sugar is…

Explanation:

Step1: Calculate molar mass of sucrose

Molar mass of ( C_{12}H_{22}O_{11} ): ( 12\times12.01 + 22\times1.008 + 11\times16.00 ) ( = 144.12 + 22.176 + 176.00 = 342.296 , \text{g/mol} )

Step2: Find moles of sucrose

Moles ( = \frac{\text{mass}}{\text{molar mass}} = \frac{30.43 , \text{g}}{342.296 , \text{g/mol}} \approx 0.0889 , \text{mol} )

Step3: Convert volume to liters

( 500. , \text{mL} = 0.500 , \text{L} )

Step4: Calculate molarity

Molarity ( = \frac{\text{moles}}{\text{volume (L)}} = \frac{0.0889 , \text{mol}}{0.500 , \text{L}} \approx 0.178 , \text{M} )

Answer:

( 0.178 )