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Ανα ~♡~
Lv 5
Ανα ~♡~ asked in Science & MathematicsChemistry · 5 years ago

Stoichiometry Question?

Update:

Consider the following reaction carried out to prepare zinc phosphate in the lab.

3Zn(NO3)2 (aq) + 2NA3(PO)4 -> Zn3(PO4)2 (s) + 6NaNO (aq)

A technician adds excess sodium phosphate solution to 5.00 L of 0.100 M zinc nitrate solution.

A) what is the theoretical yield of solid zinc phosphate?

B) If the process typically has a 97.0% yield, what mass would the technician expect to obtain when the precipitate is fully purified?

3 Answers

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  • lyssa
    Lv 4
    5 years ago

    Stoichiometry Questions And Answers

    Source(s): https://shorte.im/baqP2
  • skipper
    Lv 7
    5 years ago

    3Zn(NO3)2 + 2Na3PO4 --> Zn3(PO4)2 +6NaNO3

    5.000 L x 0.100 M = 0.500 mole of Zn(NO3)2

    0.500 mole Zn(NO3)2 x (1/3) = 0.1667 mole Zn3(PO4)2

    0.1667 mole x 320.70 g/mole = 53.45 g Zn3(PO4)2 theoretical yield

    53.456 x 0.970 = 51.85 g is a 97.0% yield

  • Roger the Mole
    Lv 7
    5 years ago

    3 Zn(NO3)2(aq) + 2 Na3(PO4)(aq) → Zn3(PO4)2(s) + 6 NaNO3(aq)

    A)

    (5.00 L) x (0.100 mol/L Zn(NO3)2) x (1 mol Zn3(PO4)2 / 3 mol Zn(NO3)2) x (386.0827 g Zn3(PO4)2/mol) =

    64.3 g Zn3(PO4)2

    B)

    (97.0% of 64.3 g Zn3(PO4)2) = 62.4 g Zn3(PO4)2

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