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Title: How do I do this limiting reactant/mass produced problem? Post by: riyaghuman on Feb 15, 2013 Ca3(PO4)2 + H2SO4 --> CaSO4 + H3PO4
What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4) by mass ? I need to understand this, not just get an answer. Thanks(: Title: How do I do this limiting reactant/mass produced problem? Post by: iliya1 on Feb 15, 2013 First, balance the equation. (You've got 6 atoms of Ca on the LHS and only one on the RHS.) Then convert masses to numbers of moles.
To do this you will need to know the molecular masses of the reagents and products; which can be evaluated by looking up atomic masses of each of the elements present, multiplying the A.M. of each element in the compound by how many atoms of that element there are and adding up. Remember also that the acid is a 98% solution; so it consists of 980 g. of H2SO4 plus 20g. ofH2O (which isn't involved in the reaction). From the balanced equation, you will see how many moles of H2SO4 you need to react with each mole of Ca3(PO4)2. The reaction will stop as soon as one reagent is used up completely. However many moles of that limiting reagent get used up will determine how many moles of each product you get. Convert moles back to mass, and there is your answer. |