Chemistry AS level question

1- It is true because one mole of any substance contains 6.02 x 10^23 particles, and one mole of H2SO4 contains 2 x6.02x10^23 of hydrogen, 1x6.02x10^23 sulfur, and 4x6.02x10^23 oxygen
2-Not true because it is not a weak acid so the concentration of hydrogen ions would be higher than the concentration of HSO4
3- Not true because sulfur contains 16 electrons and 4 oxygens contain 64 electrons
Double check tho cuz iam not a 100% sure

Can you please elaborate on the last one

Can someone pls help me ?

I would say that 1 and 3 are correct.
@Zoolato24811 reasoning is right, but i'm quite sure that statement 3 is correct as well as statement 1.

Statement 3 is correct because, 1 mole of SO4(2-) ions would have two moles of electrons. If 1 SO4(2-) ion has 2 electrons, make the ratio of 1:2.
Multiplying by avogadro's constant and you'd get that for 1 mole of SO4(2-) ions there would be 2 moles of electrons.

Like if you had 1 mole of NO3(-) ions, there would be one mole of electrons - because the ion:electron ratio is 1:1.

No statement 3 is wrong.

You say SO4(2-) ion has 2 electrons.
S has 16 protons and O has 8 protons. The ion thus contains 48 protons. By your logic the ion should have a charge of +46. Which is clearly wrong

Sulfur proton number is 16 so it has 16 electrons
Oxygen proton number is 8 so it has 8 electrons

Total number of moles of electrons = 16 from sulfur + 8 x 4 from oxygen + 2 responsible for negative charge
which is greater than 2 hence not 3

the answer is D, 1 only

Now I’m confused even more 🤣🤣so how many moles of electrons it contains

The extra 2 electrons responsible for the negative charge come from the oxygen atoms so you dont count them again.

You do. SO4(2-) contains 50 electrons.

Nope it contains 80 electrons

No.

No.

Guys I feel we have to make ionic equation out of it , when I made it for the individual ions , and added the results by making H2SO4 1 mole , there were no moles of electrons anyway , cuz the charge balances by the H+ ions

1- It is true because one mole of any substance contains 6.02 x 10^23 particles, and one mole of H2SO4 contains 2 x6.02x10^23 of hydrogen, 1x6.02x10^23 sulfur, and 4x6.02x10^23 oxygen
2-Not true because it is not a weak acid so the concentration of hydrogen ions would be higher than the concentration of HSO4
3- Not true because sulfur contains 16 electrons and 4 oxygens contain 64 electrons
Double check tho cuz iam not a 100% sure

Guys I feel we have to make ionic equation out of it , when I made it for the individual ions , and added the results by making H2SO4 1 mole , there were no moles of electrons anyway , cuz the charge balances by the H+ ions

4*16=64
1*16=16
They are joined by covalent bonds and no electrons are introduced from outside
16+64=80

They r talking about 1 mole of contains how many electrons SO4-2 contains , when H2SO4 dissociates into SO4-2, it has no moles of electrons produced with it. If we go according to what u guys are saying , why would examiner say 2 moles of electrons and make the value far from the real value

"They r talking about 1 mole of contains how many electrons SO4-2 contains"
I assume you mean
"They r talking about 1 mole of SO42- contains how many electrons"

Forget the exam question. Please answer the following questions:
(a) How many electrons does an oxygen atom have?
(b) How many moles of electrons does a mole of oxygen atoms contain?

The dissociation of H2SO4 occurs in 2 steps:
H2SO4 -> H+ + HSO4-
HSO4- -> H+ + SO42-
The first dissociation is complete as H2SO4 is a strong acid.
The second dissociation is weak because HSO4- is a weak acid. But the concentration of H+ will be greater than the concentration of HSO4- because some HSO4- will dissociate. So 2 is wrong.