What volume of CO2 released at STP on heating 9.85 g of BaCO3 ? (Atomic mass of Ba=137 ), (assuming fully decomposed)

Question

What volume of CO2 released at STP on heating 9.85 g of BaCO3 ? (Atomic mass of Ba=137 ), (assuming fully decomposed) (A) 0.84 L (B) 2.24 L (C) 4.06 L (D) 1.12 L

Tardigrade Admin · Accepted Answer

BaCO3 arrow BaO+CO2 uparrow Molecular weight of BaCO3=137+12+3× 16=197 ∵ 197 textg produces 22.4 textL at S.T.P. ∴ text9 text.85 textg produces (22.4/197)× 9.85=1.12 L at S.T.P.

Q. What volume of $C O_{2}$ released at STP on heating $9.85$ $g$ of $B a C O_{3}$ ? (Atomic mass of $B a = 137$ ), (assuming fully decomposed)

0.84 L

2.24 L

4.06 L

1.12 L

$B a C O_{3} \to B a O + C O_{2} ↑$

Molecular weight of $B a C O_{3} = 137 + 12 + 3 \times 16 = 197$

$∵ 197 g$ produces $22.4 L$ at S.T.P.

$∴ 9 .85 g$ produces $\frac{22.4}{197} \times 9.85 = 1.12$ $L$ at $S . T . P .$

Q. What volume of CO2​ released at STP on heating 9.85 g of BaCO3​ ? (Atomic mass of Ba=137 ), (assuming fully decomposed)