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How many grams of lead(II) sulfate (303 g/mol) are needed to react with sodium chromate (162 g/mol) in order to produce 0.162 kg of lead(II) chromate (323 g/mol)?

1 Answer

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Answer : The mass of
PbSO_4 needed are, 1.515 grams.

Explanation :

First we have to calculate the mole of
PbCrO_4.


\text{Moles of }PbCrO_4=\frac{\text{Mass of }PbCrO_4}{\text{Molar mass of }PbCrO_4}=(0.162g)/(323g/mole)=0.005mole

Now we have to calculate the moles of
PbSO_4.

The balanced chemical reaction will be,


PbSO_4+Na_2CrO_4\rightarrow PbCrO_4+Na_2SO_4[tex]</p><p>From the balanced chemical reaction, we conclude that</p><p>As, 1 mole of [tex]PbCrO_4 produced from 1 mole of
PbSO_4

So, 0.005 mole of
PbCrO_4 produced from 0.005 mole of
PbSO_4

Now we have to calculate the mass of
PbSO_4


\text{Mass of }PbSO_4=\text{Moles of }PbSO_4* \text{Molar mass of }PbSO_4


\text{Mass of }PbSO_4=0.005mole* 303g/mole=1.515g

Therefore, the mass of
PbSO_4 needed are, 1.515 grams.

User Adalyat Nazirov
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