AP Chemistry homework and I need help :(?
2018-02-19 12:24 pm
A sealed vessel initially contains only CO2(g) and CACO3(s). If the temp remains at 315K and the volume remains at 1.6L while the reaction bellow occurs, will the pressure inside the vessel increase, decrease, or remain the Same? Justify your answer. CaO(s)+CO2(g)---->CaCO3(s)
回答 (2)
2018-02-19 1:07 pm
The reaction is reversible, i.e.
CaO(s) + CO₂(g) ⇌ CaCO₃(s)
In the reaction vessel of constant volume, equilibrium will be finally established.
Initially, only backward reaction occurs as the rate of the forward reaction is zero because of the absence of CaO. Therefore, the equilibrium position shifts to the right. This leads to the increase in the pressure of carbon dioxide gas.
Hence, the pressure inside the vessel increases.
CaO(s) + CO₂(g) ⇌ CaCO₃(s)
In the reaction vessel of constant volume, equilibrium will be finally established.
Initially, only backward reaction occurs as the rate of the forward reaction is zero because of the absence of CaO. Therefore, the equilibrium position shifts to the right. This leads to the increase in the pressure of carbon dioxide gas.
Hence, the pressure inside the vessel increases.
2018-02-19 12:48 pm
CaO + CO2(g) --> CaCO3
in the reaction the gas CO2 is being used to form a solid. so the pressure will decrease
in the reaction the gas CO2 is being used to form a solid. so the pressure will decrease
收錄日期: 2021-05-01 22:27:27
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