July 18, 2024, 05:17:21 AM
Forum Rules: Read This Before Posting


Topic: Limiting reagents in a reaction  (Read 759 times)

0 Members and 1 Guest are viewing this topic.

Offline myicc

  • Very New Member
  • *
  • Posts: 1
  • Mole Snacks: +0/-0
Limiting reagents in a reaction
« on: June 04, 2024, 07:41:17 AM »
In the reaction represented by 3 Fe + 4 H2O → Fe3O4 + 4 H2, how many moles of H2 and what mass of Fe3O4 will be formed by the reaction of 5.10 moles of Fe?

a) 4 moles of H2 and 232g of Fe3O4 formed
b) 6.8 moles of H2 and 394g of Fe3O4 formed
c) 6.8 moles of H2 and 1.7 g of Fe3O4 formed
d) 20.4 moles of H2 and 1.18kg of Fe3O4 formed

(I got 6.8 moles of H2 by: 3moles Fe divided 5.10moles Fe ×4moles H2 = 6.8 moles of H2 and 1.18kg of Fe3O4 by 5.10x231.55 (molar mass of Fe3O4) but obviously this is not an option so I'm somewhat confused)

Offline mjc123

  • Chemist
  • Sr. Member
  • *
  • Posts: 2068
  • Mole Snacks: +302/-12
Re: Limiting reagents in a reaction
« Reply #1 on: June 04, 2024, 09:00:38 AM »
Why 5.10 x 231.55? If you have 5.10 moles Fe, how many moles of Fe3O4 do you get?

Sponsored Links