Chemistry work help asap

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    piece of zinc was added o 50.0cm^3 of 2.00 mol dm-3 sulfuric acid (an excess). The zinc reacted according to the equation:

    Zn + H2SO4 ---> ZnSO4 + H2

    The remaining sulfuric acid required 27.50cm^3 of 0.200 mol dm-3 sodium hydroxide for neutralisation.

    2NaOH + H2SO4 ---> Na2SO4 + H2O

    1) Calculate the number of moles in 50.0cm^3 of 2.00 mol dm-3 sulfuric acid
    2)Calculate the number of moles in 27.50cm^3 of 0.200 mol dm-3 of sodium hydroxide
    3) use the second equation to calculate the number of moles of sulfuric acid remaining after the reaction with zinc
    4) Use your answer from parts (1) and (3) to calculate the number of moles of sulfuric acid which reacted with the zinc
    5) Hence calculate the mass of zinc that reacted
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    I refuse to do your homework.

    I will help you, but not just do it for you.

    Why can't you do it?
 
 
 
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