Calculate the mass of each product formed when 228 g of silver sulfide reacts with excess hydrochloric acid.
Ag2S(s) + HCl(aq) AgCl(s) + H2S(g) [unbalanced]

Question

Calculate the mass of each product formed when 228 g of silver sulfide reacts with excess hydrochloric acid.
Ag2S(s) + HCl(aq)  AgCl(s) + H2S(g) [unbalanced]

wolfe8 · Answer

1) Balance the equation
2) Find the number of moles of silver sulfide used
3) Look at the equation and find the number of moles of the products
4) Convert to mass

anonymous · Answer

blahhh i cant balance it. the Cl is not being nice!

wolfe8 · Answer

But it's the same equation as before O.o

anonymous · Answer

NVM i wrote it a way i didnt see the 2!

anonymous · Answer

there is one mole os Ag2S.

2 moles of AgCl and 1 Mole of H2S!

wolfe8 · Answer

Alright so do what we did before.

anonymous · Answer

228/ 247.87 correct?

wolfe8 · Answer

Yup

anonymous · Answer

then multpily by the moles and the molar mass?

wolfe8 · Answer

Of the respective product, yes.

anonymous · Answer

for AgCl i got 263.7

wolfe8 · Answer

Yup

anonymous · Answer

THanks dudeee. hahah you are surely gonna get alot of medals from me :D

i understand it now!!!!

wolfe8 · Answer

Lol. No problem. That's what I'm here for.