How many milliliters of carbon dioxide gas at stp are produced from the decomposition of 1.52 g of lithium hydrogen carbonate?
2lihco3(s)→li2co3(s)+h2o(l)+co2(g)

Molar mass :

CO₂ = 44.01 g/mol
LiHCO3 = 67.95 g/mol

Mole ratio: ( Calculate the mass of CO₂ ) :

2 LiHCO₃(s)→Li2CO₃(s)+H₂O(l)+CO₂(g)

2 x 67.95 g LiHCO₃ 44.01 g CO₂
1.52 g LiHCO₃ ??

Mass of CO₂ = 1.52 x 44.01 / 2 x 67.95

Mass of CO₂ = 66.8952 / 135.9

= 0.4922 g of CO₂

Number of moles:

mass CO₂ / molar mass CO₂

0.4922 / 44.01 => 0.01118 moles of CO₂

1 mole 22.4 L ( at STP )
0.01118 moles ??

0.01118 x 22.4 / 1 => 0.250432 L

Therefore:

1 L 1000 mL
0.250432 Volume

Volume = 0.250432 x 1000

= 250.432 mL

You are welcome! =)

The answers are 3.c kelvin4.b liquids only