Question

a) How many grams of pure CaCO3 is required to produce 1 L of CO2 at 270C and 750 mm of

pressure?

b) A solution of hydrochloric acid contains 22% acid by weight. How much of this acid is

required to produce 1 L of CO2 at 270C and 760 mm of pressure? (Ca = 40, C = 12, Cl = 35.5)​

Answer 1

Answer:

CaCO

3

+2HCl→CaCl

2

+H

2

O+CO

2

100 g 44 g

1 mole 1 mole

22.4 L 22.4 L

We know that 1 mole of any gas at 0

o

C and 1 atm pressure occupies 22.4 L volume.

So, 100 g CaCO

3

forms 22.4 L of CO

2

Hence, 2.5 g CaCO

3

will form =

100

2.5×22.4

=

100

56

L of CO

2

=0.56 L of CO

2