## E. 23

Qining Jin 1F
Posts: 53
Joined: Fri Sep 29, 2017 7:07 am

### E. 23

Question:
Calculate the amount (in moles) of (a) Cu2 ions in 3.00 g of CuBr2; (b) SO3 molecules in 7.00 x 10^2 mg of SO3; (c) F ions in 25.2 kg of UF6; (d) H2O in 2.00 g of Na2CO3 10H2O.

Hey can someone show me how to set up part a? I seem to be having a brain fart...

Golbarg Rahimi 3k
Posts: 26
Joined: Sat Jul 22, 2017 3:01 am

### Re: E. 23

you have 3.00 grams of CuBr2 with the molar mass of 223.35. by dividing them you get the moles of CuBr2 available. each mole of CuBr2 has 1 mole of Cu ions.
therefore the number of moles of CuBr2 equal the number of moles of Cu ions .

Qining Jin 1F
Posts: 53
Joined: Fri Sep 29, 2017 7:07 am

### Re: E. 23

Oh my gosh I wrote down CuBr3 instead of CuBr2. Thanks!

Kyla Roche 2D
Posts: 42
Joined: Wed Sep 30, 2020 9:59 pm

### Re: E. 23

For part c, I got the molar mass of the UF6; however to find the amount of F ions I am unsure of the next step to take if someone could please help me!

Shruti Kulkarni 3G
Posts: 45
Joined: Thu Oct 08, 2020 12:16 am

### Re: E. 23

Hi Kayla! After finding the molar mass you can convert the grams of UF6 to moles and then do the molar ratio. In every mole of UF6, there will be 6 moles of F ions, since there are 6 F ions in every molecule of UF6. Knowing the molar ratio you can solve for F ions.