If 60.0 grams of carbonic acid are sealed in a 2.00 l soda bottle at room temperature (298 k) and decompose completely via the equation below, what would be the final pressure of carbon dioxide assuming it had the full 2.00 l in which to expand? h₂co₃(aq) → h₂o(l) + co₂(g)

The final pressure of the carbon dioxide gas will 11.84 atm.

Explanation:

Moles of carbonic acid =

According to reaction, 1 mol of carbonic acid gives 1 mole of carbon dioxide gas.

Then 0.9677 moles of carbonic acid will give :

of carbon dioxide

Moles of carbon dioxide gas = n = 0.09677 mol

Volume of soda bottle =

Pressure of the carbon dioxide gas = P

Temperature of the carbon dioxide gas = T = 298 K

(ideal gas law)

The final pressure of the carbon dioxide gas will 11.84 atm.

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation: