What volume of carbon dioxide measured at 27^(@)C and 746.7 mm pressure would be obtained by treasting 10.0 g of pure marble with dilute hydrochloric acid ? (Aq. Tension at 27^(@)C is 26.7 mm).

What volume of carbon dioxide measured at 27^(@)C and 746.7 mm pressur

1.	What volume of carbon dioxide measured at 27^(@)C and 746.7 mm pressure would be obtained by treasting 10.0 g of pure marble with dilute hydrochloric acid ? (Aq. Tension at 27^(@)C is 26.7 mm).
Answer» Solution :The CHEMICAL equation representing the reaction is : `underset(100 g)(CaCO_(3))+2HCl rarr CaCl_(2)+H_(2)O+underset(22400 cm^(3)at STP)(CO_(2))` STEP 1. To calculate the volume of `CO_(2)` evolved from 10 g of `CaCO_(3)` at step. From the chemical equation, 100 g of marble react to produce `22400 cm^(3)` of `CO_(2)` at STP `therefore 10 g` of marble will produce `CO_(2)(22400)/(100)xx10=2240 cm^(3)` This is the volume of `CO_(2)` evolved at STP. Step 2. To calculate the volume of `CO_(2)` at `27^(@)C` and 746.7 mm pressure `{:("Initial conditions","Final conditions"),(V_(1)=2240 cm^(3),V_(2)= ? cm^(3)),(P_(1)=760 mm, P_(2)=746.7-26.7=720 mm),(T_(1)=273 K,T_(2)=27+273=300 K):}` APPLYING the gas equation, we have `(V_(2)xx720)/(300)=(2240xx760)/(273)` `V_(2)=(2240xx760)/(273)xx(300)/(720)=259.8 cm^(3)` Thus, the volume of carbon dioxide obtained `= 2598.3 cm^(3)`.