Red #40 has an acute oral ld50 of roughly 5000 mg dye/1 kg body weight. this means if you had a mass of 1 kg, ingesting 5000 mg of red #40 will have a 50% of killing you. determine the amount of dye a 70 kg person would need to eat to reach his or her ld50. how many moles of dye would that be? the molar mass of red #40 is 496.42 g/mol. using the calculated concentration of red #40 dye in the sports drink, how many of liters of sports drink would it take to reach this ld50?

350 g dye

0.705 mol

2.9 × 10⁴ L

Explanation:

The lethal dose 50 (LD50) for the dye is 5000 mg dye/ 1 kg body weight. The amount of dye that would be needed to reach the LD50 of a 70 kg person is:

70 kg body weight × (5000 mg dye/ 1 kg body weight) = 3.5 × 10⁵ mg dye = 350 g dye

The molar mass of the dye is 496.42 g/mol. The moles represented by 350 g are:

350 g × (1 mol / 496.42 g) = 0.705 mol

The concentration of Red #40 dye in a sports drink is around 12 mg/L. The volume of drink required to achieve this mass of the dye is:

3.5 × 10⁵ mg × (1 L / 12 mg) = 2.9 × 10⁴ L

c. because step up transformer steps up the input voltage i.e increases the input voltage  

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transformer does not handle dc current