10g lime stone when reacts completely with dilute HCl it produces Co, gas.If the reaction happens at 27°C, 780 mm pressure then calculate the volume of that gas? (Ca=40, C=12, 0=16]
Answers
Answer:
0.56 L of CO
Explanation:
CaCO
3
+2HCl→CaCl
2
+H
2
O+CO
2
The volume of CO
2
gas formed when 2.5 g calcium carbonate is dissolved in excess hydrochloric acid at 0
o
C and 1 atm pressure is:
[1 mole of any gas at 0
o
C and 1 atm pressure occupies 22.414 L volume].
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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
Explanation:
10g of CaCO3 is 10/(40 + 12 + 3x16) = 0.1mol. So the equation is:
0.1CaO3 + 0.2HCl = 0.1CO2(g) + CaCl2 + H2O(l)
Change in Free Energy ΔG(20C) = -6.0kJ (negative, so the reaction runs)
Change in Enthalpy ΔH(20C) = -0.35kJ (negative, so the reaction is exothermic)
So, 0.1mol of CO2(g) is produced, which is 4.40g or 2.24L