Complete the balanced equation for the overall reaction in a hydrogen fuel cell. _ H2 + ___ > _ H2O

Hydrogen fuel cells are really important as they can be used to power electrical cars, so it's something that a lot of scientists are looking into at the moment. We need to balance this equation, so we need the same amount of things at the begining, in the reactants, as we do at the end, in the products. We have that Hydrogen (H2) and something are making water (H2O), so the thing that is in the product that isn't in the reactants is Oxygen (O2). This gives us _H2 + _ O2 > _H2O, so now we need to make sure we have the same amount of each element in the reactants and products. If you tally up the number of H and O at the start and the end you see we need more oxygens in the product. Overall we have 2H2 + O2 > 2H2O

Answered by Kyra B. Chemistry tutor

6429 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

What are the differences between the effects of a catalyst vs reactant concentration on the position of equilibrium/ why?


What is the concentration of 0.4 moles of 25cm3 ethanoic acid?


How do you test for the different halide ions?


What is the conservation of mass and what does this mean in relation to equations?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo
Cookie Preferences