Limiting reactant: What mass of water `(H_(2) O)` can be formed by the reaction of `3.00g` of `H_(2) (g)` with `29.0g` of `O_(2)(g)`?
Strategy: Using the balanced equation
`{:(2H_(2)(g),+,O_(2)(g),,rarr2H_(2)O(l)),(2mol,,1mol,,2mol),(2(2.00g),,32.0g,,2(18.0g)):}`
find out the numbers fo moles of each reactatn required to react with the other. Using the given masses, calculate the number of moles of each reactant. Finally, identify the limiting recatant and base the rest of the calculate on it.