Question

If anyone could help I’d appreciate it

Answer 1

Answer: 2.00 mol

Step-by-step explanation:

The balanced chemical equation is:

`2H_2(g)+O_2(g)\rightarrow 2H_2O(g)`

According to stoichiometry :

2.00 moles of
`H_2` require = 1.00 moles of
`O_2`

Thus 2.00 moles of
`H_2` will require=
`(1)/(2)* 2.00=1.00moles` of
`O_2`

Thus both will act as limiting reagents and will be fully consumed.

2.00 moles of
`H_2` will form = 2 moles of
`H_2O`

Thus 2.00 moles of
`H_2` will form =
`(2)/(2)* 2.00=2.00moles` of
`H_2O`

Thus 2.00 moles of
`H_2O` will be produced from the given masses of both reactants.