45 How many kg of CaCO3 is needed to produce 336 kg of CaO , if % yeild of the reaction gives is 60% . CaCO3 -> CaO + CO2

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Solution

The decomposition reaction of calcium carbonate is given as:
$C a C O_{3} (g) ⟶ C a O (g) + C O_{2}$
$100 g m 56 g m$
One mole of calcium carbonate decomposes to give one of calcium oxide and carbon dioxide each.
For 100% yield, 56 g of calcium oxide is formed.
So for 60% yield, the amount of calcium oxide formed is
$100 % ⟶ 56 g m o f C a O$
$60 % ⟶ x g o f C a O$
$x = \frac{56 \times 60}{100} = 33.6 g$
So with a percentage yield of 60%, 100g of calcium carbonate gives 33.6 g of CaO
So the amount of calcium carbonate needed for 336 kg of calcium carbonate is:
$100 g m o f C a C O_{3} ⟶ 33.6 g m o f C a O$
$x g m o f C a C O_{3} ⟶ 336 K g o f C a O$
$x = \frac{100 \times 336 \times 10^{3}}{33.6} = 10^{6} g = 10^{3} k g$

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Calculate the amount of $C a C O_{3}$ (m wt = 100 gm/mole) is need to produce 336 kg of $C a O$ (m. wt = 56 gm/ mole), according to reaction:

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