Question

Using the balanced molecular equation below, determine the grams of solid that would form if you started with 17.13 grams of CuSO4?

3CuSO4 + 2Li3PO4⟶3Li2SO4 + Cu3(PO4)2


Record your answer to 2 decimal places

Answer 1

produced solid mass = 13.62 grams

Step-by-step explanation:

By assuming that
`Li_(3)PO_(4)` is excess and knowing the fact that
`Cu_(3)(PO_(4))_(2)` is insoluble in water, which will be the yielded solid

Molar mass of CuSO4 = 63.5 + 32 + 4(16) = 159.5 g/mol

Moles of the Reactant copper sulphate
=
`(17.13)/(159.5)` = 0.1074 moles

by putting given data in ratios:

3CuSO4 + 2Li3PO4⟶3Li2SO4 + Cu3(PO4)2
(3) : 2 : 3 : 1
(0.1074) : --- : --- : ?

Part value = 0.1074/3 = 0.0358


`Cu_(3)(PO_4)_2` moles = 1 * 0.0358 = 0.0358 moles

molar mass of
`Cu_(3)(PO_4)_2` = 3(63.5) + 2(31 + 4(16)) = 380.5 g/mol

moles of
`Cu_(3)(PO_4)_2` = 380.5 * 0.0358 = 13.62 grams

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