following calculation, giving the answer in the correct number of significant digits. (1.145 x 109 g/mol) (0.0035 mol)/(8.57 x 10 g/mL)-_4.6x102 mol/ml (145X10Zlmai) (0.0035mo1) 8.5x10g/mL 2. Convert the following amount to kJ. 34.5 J 0.0345 1 kJ = 34.5Jx 1090 J 3. An experiment calls for 7.57 g of sugar. You have a sugar solution that is 5.00% by weight (for every 100 g of solution, there are 5.00 g of sugar). How many mL of the sugar solution will be needed to deliver 7.57 g of sugar? The density of sugar solution is 1.157 g/mL. The molecular weight of sugar is 342 g/mol. ImL ? mL = 7.579 x = 6,54 mL 312 7.57 g suur x 1.157 1,157 bin= b az lot volume of solution - 6.54 ml