Question #246955

How much of Ti, in g, should be obtained to have 94.97% yield?


1
Expert's answer
2021-10-08T02:08:46-0400

Let’s us the following example.

Titanium metal can be obtained from its oxide using the following chemical reaction:

TiO2(s) + 2C(s) → Ti(s) + 2CO2(g)

28.6 kg of C reacts with 88.2 kg Ti(IV)O. How much of Ti, in g, should be obtained to have 94.97% yield?

M(TiO2) = 79.86 g/mol

n(TiO2) =28.6×10379.86=358.12  mol= \frac{28.6 \times 10^3}{79.86} = 358.12 \;mol

According to the reaction one mole of Ti is obtained from one mole of TiO2.

n(Ti) =n(TiO2) = 358.12 mol

M(Ti) = 47.90 g/mol

m(Ti) =47.90×358.12=17154.27  g=17.154  kg= 47.90 \times 358.12 =17154.27 \;g = 17.154 \;kg (theoretical 100% yeild)

Proportion:

17.154 kg – 100 %

x kg – 94.97 %

x=17.154×94.97100=16.291  kgx = \frac{17.154 \times 94.97}{100} = 16.291 \;kg

Answer: 16.291 kg


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