Chem helpppp

Some people are concerned that aspartame, C14H18N2O5 may have adverse health effects.

Research shows that the safe maximum daily intake of aspartame is 1.7 x 10^-4 mol kg^-1

A typical adult has a mass of 75kg
A can of diet drink contains 167mg of aspartame

How many cans of this diet drink is it safe for a typical adult to drink in one day?

I don’t know how to answer this question can someone please help!!

Chemistry help

Reply 1

Pyruvic Acid

17

What have you done so far?

Reply 2

Unknownn1.x

OP

8

Original post by KaziMahathir

What have you done so far?

Literally nothing, I don’t know what to do at all

Reply 3

Pyruvic Acid

17

Original post by dayaaa.x

Literally nothing, I don’t know what to do at all

I think the key to success in this question is breaking everything down into smaller steps. The first thing I would do is work out the total number of moles of aspartame that a typical adult can take by multiplying 1.7 x 10^-4 mol kg-1 by 75kg. This would give us a total of 0.01275 moles.

The second thing I would do is calculate what mass this equates to, seeing as the amount of aspartame in the can is expressed as mg. This is done by using the formula n = m/Mr or n x Mr = m = 0.01275 moles x 294.3gmol^-1= 3.752325g.

The third thing I would do is convert this value from g to mg by multiplying by 1000 to get 3752.325mg. Finally, we would divide the total mass of aspartame that a typical human can take in one day by how much is in a can (e.g. 3752.325mg by 167mg) which would give us 22.47 cans.

We then round this down to 22. Hopefully, I haven't made any errors in my method :biggrin:

(edited 3 years ago)

Reply 4

Unknownn1.x

OP

8

Original post by KaziMahathir

I think the key to success in this question is breaking everything down into smaller steps. The first thing I would do is work out the total number of moles of aspartame that a typical adult can take by multiplying 1.7 x 10^-4 mol kg-1 by 75kg. This would give us a total of 0.01275 moles.

The second thing I would do is calculate what mass this equates to, seeing as the amount of aspartame in the can is expressed as mg. This is done by using the formula n = m/Mr or n x Mr = m = 0.01275 moles x 294.3gmol^-1= 3.752325g.

The third thing I would do is convert this value from g to mg by multiplying by 1000 to get 3752.325mg. Finally, we would divide the total mass of aspartame that a typical human can take in one day by how much is in a can (e.g. 3752.325mg by 167mg) which would give us 22.47 cans.

We then round this down to 22. Hopefully, I haven't made any errors in my method :biggrin:

Thank you so much!!!! :smile:

this really helps i understand now

Reply 5

Amy332033

7

Original post by Pyruvic Acid

I think the key to success in this question is breaking everything down into smaller steps. The first thing I would do is work out the total number of moles of aspartame that a typical adult can take by multiplying 1.7 x 10^-4 mol kg-1 by 75kg. This would give us a total of 0.01275 moles.

The second thing I would do is calculate what mass this equates to, seeing as the amount of aspartame in the can is expressed as mg. This is done by using the formula n = m/Mr or n x Mr = m = 0.01275 moles x 294.3gmol^-1= 3.752325g.

The third thing I would do is convert this value from g to mg by multiplying by 1000 to get 3752.325mg. Finally, we would divide the total mass of aspartame that a typical human can take in one day by how much is in a can (e.g. 3752.325mg by 167mg) which would give us 22.47 cans.

We then round this down to 22. Hopefully, I haven't made any errors in my method :biggrin:

where did u get the 294.3 from ??