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 cold front replaces the warmer air at the ground level changing the wind to be breezy and denser.there is also an immediate drop in the temperature.

chemical changes occur when a substance combines with another to form a new substance, called chemical synthesis or, alternatively, chemical decomposition into two or more different substances. these processes are called chemical reactions and, in general, are not reversible except by further chemical reactions. some reactions produce heat and are called exothermic reactions and others may require heat to enable the reaction to occur, which are called endothermic reactions. understanding chemical changes is a major part of the science of chemistry.