. Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide was collected at 27oC and normal pressure


Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide was collected at 27oC and normal pressure.

Calculate:

(a) The mass of salt required.

(b) The mass of the acid required to prepare the 2 litres of CO2 at 27 C and normal pressure.

CaCO3 + 2HClCaCl2 + H2O + CO2

 

Best Answer

CaCO3 + 2HCl→CaCl2 + H2O + CO2

100g73g22.4L

(a)V1 =2 litresV2 =?

T1 = (273+27)=300KT2=273K

V1/T1=V2/T2

V2=V1T2/T1mass

Now at STP 22.4 litres of CO2 are produced using CaCO3 =100g

So, masslitres are produced by =100/22.4 2274/300 =.125g

(b)22.4 litres are CO2 are prepared from acid =73g

masslitres are prepared from = 73/22.4 2273/300=5.9g

 

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